SCIENTIFIC ABSTRACT TANANAYEV, I.V. - TANANAYEV, I.V.

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• Collection: Scientific Abstracts
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• Release Decision: RIF
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• Document Page Count: 100
• Document Creation Date: November 2, 2016
• Document Release Date: July 13, 2001
• Sequence Number: 7
• Publication Date: December 31, 1967
• Content Type: SCIENTIFIC ABSTRACT

Ud--,jR/dhiisiatrY: Lead Th6orium `~2,
Systems
"Physico-chemical Analysis of Systems of Importance
to Analytical Chemistry. XX. TheL Solubility of
Iliecipitates in Complex (Really Existing) Anklyti-
cal. Systems," I. V. Tananayev, I. B. Misetskaya,
A.' D. Vinogradova, InSt of Gen and Inorg,Chem, AcaA
Sci USSR
."Zhur Arialit Xhim" Vol VII, No 1, py 14-20
Studied soly in the system PbSO4 -. Th(NO - Li Soh-
a ? 2
0 at 250C. The Debye-Rueekel formu.1 or caleg
Nte soly of PbSO4 is not suitable for this system,
because of the marked chem interaction accompanied
209T8
USSR/Chemistry Lead, Theorium Jan/Feb 52
Systems (Contd)
2+
by formation of ions of the type ThS02 . -Considers
the 't-hi,oryn
of pptn reactions, and a diagram shoit
the following types of ternary systems: ypt -
electrolyte with common ion - water, embracing all
possible systems vith ppts in dependence on the ion
type of the components and the character of the
process of interaction in the system.
(CA 41 h*.-Iq;q?4q

TANAMYNY. I.V,; GWSHKOVA, M.A.; SITYER, G.B.
Chemistry of lanthanum forrocyanides and their application in ana-
lytic chemistry. Khtm.redk.elem. no-1:58-86 154. (KM 8:3)
1. Institut obahchey i neorganichaskoy khImil Im. N.S.Xurnakova
AN SM -
(Lanthanum ferrocyanide)

TAILNAYW, I.V.; IMYCM4AN, B.N.
3 the solutions of indium fluoride andL oxalate. M21m.
rodk.elem. no-1:87-94 154. (MM 8:3)
1. Inatitut obshchey i neorganicheskoy khimii im. N.S.Eurnakova
AN SM.
(Indium salts)

Ad*ii1T" A d1j T _.7
m
A
k~
.
en
a
v,
g- lot

n in
ot 30 g. 100 11;Melt with
gentle In the ptevnca oI H304; (allowed
'
Alon of I.M, 11A. cohm
, washing of the t)pt. with 50%

art
EtOH d.air-drying 2-3 days gave: colorless rnI7i.3LrG,
tetrag at Prfstim, no 1.460, na 1.427, sot. in 11,0 (5.8%
at 25* 1 Sol. in HCI and, 11NOl, less sot. in Ht,904; reacts
with NaOll but gives no ppt. with CaCI: The x-my dia-
gram Is given'l Oi!,P,Wt ogl,,the&It sl;owq endothermic
k.'Usr stleorresponds to loss of
effects at~Hqrffi Ilifn
_
4H.0 dfid Zklify- tllt%lid top loss of 1110 ancl HF-to, form
FA'
Alle'
T
I
r
l
kit
f
N
V
11
t 25% b
-
.
l-
n
a
ein
ow
%
n
a
e
l a
MIF supersutd. solns. are fornied; 1001-130 Is the solid
phasm. At 0.150, NaP and 9.89% InFj therearc formed
InF, and 3W.103; at Nal? conens. up to 2.5, the solid
phase Is 3NdF.[,n& somewhat sot. in MOIL sot. in FICI,
TINOs and H30, yielding a ppt. with CaCII. - Its x-ray dia-
grant.differs considerably froin that of NaP or Itirs-314to.
shom
3NaP.1ur endothermic effects at M., SM, rind 870%
possibly caused, I)y.partW 10.13. of F. the c6inpIq thelts
above 1000*. toNWdP4M;j._

~~ _A

physleachemical rMlysts ~of s St&MS I Va ut- a
Y
r
UUM --jrXKV. To y actiOil Of tOMd-:!
of to,
d
u
Y
lion
l
fdUiinur~ ~Yiroxldo by we"Utulnent of tho it arent
of the precipit4tec. L V. Tanatiaev and"91. A.:-
0 Va. '~M anal.: ghfinq Mid. Neuk
TrIf4y IF
U's S_ 10luslik..

-F, --.- - --- - ' - Ah N40 Z(B), M-53(lQ54); rf. (ut,
w
T- qur.'711101. stq.
147 Is -Thc npliiftrit vol. ill the
03
ipf, 48, 8011 M, i~
f to - plitit. of Al(OFI)~,' The M. ill ppt~ I's Plotted
't.
d
y tht
2gainst the ratio 011.Al in the or164nal wixt, Cathonute-1
IreeNA011 soln., and AKNO,~ and AIASO), vins. contg. tit) I
ift. 464 were vicd. Into a 2&-jnl duated tube intro-i
duct the At whi 140, and KaOH, i such (tuits. Iluit after!
adkin. of,the NaOlf th.- vol, 6 25 mt. Stapptr the who and
-they) invext approx, 200 flints.: After a dad. interval reud
..the upper butindary of the ppt. In expts..Avith const. At
,
eontent-(0,01-0.0U, f) Rpm of plit. begins when the rat
011:Alisapprox.2.4. Thecurvehasa max. utOMAI - 3.~
*
-,m 2.8, At cannot
bc detected in sriln. and the vnl, i
AtOH:Al
txiu& less than at 0111 At ~w 3. At 011: A m
of
t s
1
v
v, at ;1~
0 , 4,theppt~d1&solvesccnnpJetdy. Aftcribr.the-
g

-~" thax. could benotitedclearly. After24tim.thevol.ofEpt.~
- A
h
a
]A fterseveral hrg.
*L4 Const.
t roota tenip. the ppis w ic
;
ed with 011 -At > 3 became whiter but the others t
_rstart out
corticd HC1 is added to each tube I
-,didnotchange. Ifl-2tal.,
d i ed th ppts. forined witit 0H:AI < 3 quicki,
an ml;. , e r dis-
'A
Mlvi- b A the others remain lasol. for 24 lira. . In ~~ts-
I
where the sum. of:AI(N%)z and NaOll conchs. alwaysi
equglied 0.1,11', addn~ of NaN(h (0,6 and IM) briore, the;
NALOR does not ih."ge the gencral outfini, of the curve but
ta..beghistarlier. With: the- systeta Al(N0j),-Nffj0II-
but ife-
the ppt.,Is a max.. tit OU:A,I._.

r
INgYM4E
crvascs slut ly whea,iviore NMOIT is uddal.' When Nllia- 7
rp
bcforeNlT,0H thismax.1stlis-',
placed to the left immediately after pptn. but on standing
Yre%torcs the max. to 0H-.AI 3. At NlIsNO, IM the
inax. is displaced alightly. to the right and vol. of ppt. does;
incittlecrmsesosli-.trljly.wlttitcxt=NH4OHisaddW, Pptn. ' ~,.: ,
occurs earlier than Qlr-.Al - 2. With Af~604~ - 0.011f,~ 'e F
irtud N-.kOlt,pptti.lx-giiisnppr6x.wliemitdnes with AI(Nos)#.
'I'llerl 2max. arc obwved. at 011:A1 m 2.5 and at 3, witha
min. betiveen them. 'The min. develops more clearly -by
aging. With A14604h = 0;02AI and with NuCtUt them Is
only 1 max. at 2.5. . Iror A1004s 0.(k2JV and with
NFLOR, the first max remains the same but second tna%.is,'
lesssharp.
Hj0 with AI(NOj)~ w 0,04M., With no sulfate pptn. begins
at OMM - 2.5. With 0.002,V of (NIIt)sS0, added the
ppL. is stable at 0MAI -~ 2 mud the vol. is larger. .'The
MaXASSWIFILM With (NH4M04 at 0.01AI this max. is at
2,6--2.7 and a very weak secood'atak.As displaced to the,
rrisht.* At - 0.03M, the fma mat. is at,2.6-~2.7
atutthesmond max. ir more noticeable.! At CNU4)*SO4
0.3.1f the first max. is at 2.5 and the $Mand max dis-
appwars. In significant conen. of sulfate the max, v~l. Of.
ppt. is obtained at a point corresponding to a basic salt. 10.
-olu. -it
Al(0JJN.Al*(S0,),~ No A) ions arc,delected in
2A.. Existence- of second max,depends on many
conditlowq. It is suggested that with a large, cxms ofAll~`
the ions AI(011)"+ and AI(Oll),* are formed, with -Anall
-"CCS$ of All' oilloidai Al(011h is formed. Sinerevenin
the presence Of electrolytvs, AI(Otf)s is not st:pd. earlier-
thau OH: At - 2. that vulue may be the boundary between
the fortits, *ne intvrinedia(c stage would be a colkAAA
11ticelle, [A1(0ll),j.,jA1(0lI),+j.Cl-, Nr N4011 rfr MGM
-ystems. AvO-~ F-, and malate cautsc caly ppla. of M.
In Ilke icl)tl. -Ir AV- ai Al((,)11), frOla bi%-3ltUt Vikti(YaS IW
I LICI
3-11111. Of XaOAc, nO exv,:-,,f N.%OAc colipti. ilie-lviv; ;1'
i.,t;q. Adda, of;L lit thea c-ir,ftfl ttoitnfira,'+
6-1 .,f the fr,,I- avill i, Mayelle

/VA
GRINBERG, A.A. (Leningrad); BABAYEVA, A.V.(Moscow); YATSIMIRSKIY. K.B.
(Ivanovo); GORNKYKIN. V.I. (Moscow); BOLIY, G.S. (Moscow); FIAL-
KOV. Ya.A- (Kiyev); YAKSHIN, M.M. (Moscow); XUR V. B.M. (Moscow);
GILOUN, A.D. (Moscow); 73DOROV, I.A. (Moscow); PANSIKYUK, Ye.A.
(Leningrad); VOLIKENSHTZYN, N.V. (Leningrad); ZHDANOV, G.S. (Moscow);
PTITSYN, B.V. (Leningrad); ABLOV, A.V. (Kishinev); VOLSHTM, L.M.
(Dnepropetrovsk); TROITSKAYA, A.D. (Kazan'); KIOCHKO, M.A. (Moscow);
MARAYNTA, A.V.; TRONIV, V.G. (Moscow); RUBINSHTZYN, A.M.(Moscow)
CHERSTAYN, I.I.; GRISBZRG, A.A.; TANANATIV, I.T.
31rplanation of the tranneffect. Isv.Sekt.plat.i blag.met. no.28:
56-126 154. (MLBA 7:9)
(Compounds, Complex) (Platinum)

TANIANAYJ~, I. V. rind N. V.
"On the Formation reaction of gallium hydroxide", Khimiya RedIkikh Elementov,
No. 2, ~,12, 1955.
The mechanism of the formation of gallium hydroxide was investigated by a
study of the system GaC13-NaOH-H2O. The measurements of solubility, liaht
~absorrtion and volumes of precipitates were used for the investigation. The
reaction takes place in five stages, depending on the molar ratios of NaOH to
GaGl in the initial mixture, with the suecessive formatidn of Ga(OH)'12,
Ga(a)2C121 Ga(OH)2C' (soluble basic salts), Ga(OH)2.8ClO.2 (insoluble
basic sal ), Ga(OH)3 and then soluble gallate.
SO: D-1~13171

TANANAY3V,_I. V. and BAU507-A, N. V.
"A study of the chemistry of gallium fluorides and their utilization
for the separation of gallium from other metals", Kh:Lmiya Redkikh Elementov,
No. 2, p 21, 1955-
A method of preparation of GaF 3H20 by the action of hydrofluoric acid
on metallic gallium. The reaction beKeen GaU ~ and HF in aqueous solutions
was investigated, the 'Lormation of a stable ZP2, ion was established.
Solubility in the system: GaF3-NaF-H20 at 25'C was investig-,'ted. The formation
of a double salt of the composition 13NaF. 5GaF 30 practically insoluble in
sodium fluoride solutions was established. On the basis of the latter a method
of quantitative precipitation of -gallium. from Zn, Co, Ni, W, Mo, Cd and Cu
was developed.
SO: D-413171

.............
TANANAYEV, L"1. and S. N.
"On indium ferrocyanides", Khimiya 9edkikh KLementov, No. 2, P 37, 1955.
The systems: InCl Li Fe(CN)b-H 0- INC1 -Na Fe(CN)6H2O and
3 - 4 2 )
INC13-K4Fe (CN)6-H20 were investigat6d using solubiii-ty electroconductivity,
potentiometrie and turbidometric methods. Concentrations of components were
those used uncer normal analytical conditions. It was found that in the first
two systems indium ions react forming salts of the normal composition In
fFe(CN)673 and in the third system, in addition tothe normal, a doubl~4salt
is formed uncer certain conditions.
SO: D-413171

d cerium 1. V. Tagn-Bev
G. vwsgmul zhlir' 11 i.' I.* i4a. I. D4-,%,R 17M
C111 Cc(NO, LL -w- I
Ort(CN)*1 If with'CL
D. I n
(NOA2 conca. Initially at 0. mol,/I., ad n. of L�4[Fc
(CN causes stoiclAometric pptn. of CcdfFC(CN)sh.-
2OUX (1), whose tiWr soly. at 25'.=6 O.t* is 1.3 X 10-6
m0leff. In the system Qe(NOj)j-Na4jFe(CN~j"ffgO,
IispPtd. initially, If Na4lFe(CN)s) Is added In excewthe.
solid phase becomes NaCej[Fc(CM)sh.XJI'O, whose Say.
is 2.1 X 10-4 mole/l.. In the system Y(N%),-K&[Fe-
(CN)sFlf,Oj~ only K4V8fFe(CN),b.30ffjO ppts, soly. 6.2.
X 10-6 mole/I.). In the system CH ACN)s),
HrO the ppt. is KCtjFe(CNN).21ItO (soly. 2.4 X 10-4
In Y(N%),PNjFe(CN),j-HO only RbV-
e
CNM-21-10 is pptd. (soly. 1.8 X 10-4 rnole/L). In
(
W%)~-Rb4[Ve(CN~J-11tO the ppt. Is RbCe(Fe(CNI~J.w-
-.*0 (soly. 7.1 X 10-4 moleA.). In Y(NO.)rCs.[Fe- It
(CN)#~-HO the ppt, is Csy[Fc(CN).
tall"O (Soly. 5.2 X
10-6 wo".). In Ce(N%)~-"(Fe( N)*FHIO. the ppt.
is CsCe[Fe(CNM.2If,O (soly. 1.7 X 10-1 mole/I.). In
the systems Y(NO,)r-L4(Fc(CN)gF.H3O and Y(N%)r-
Na4[Ft(CNhl-HiO.noYfeiTocyanideispptd. Itisthere-
fore suggesied that pptn. svith MajjFetCNhj or L4(Fe-
CN)'j nULY be useful in Sept. Ce from Y. C. It- F.

1 fl-N --":, - - - . . I - . 1.
! 7 f.4 v
I~N -P;v

- U -V-

J
1--lhe fo=gi~an of 1. V. Tananaev
an, N 0 'H"'Ml,
(19mT. r- Wit M'S wa3 -itudled by
the ructh(As of Eoly., j,v cit"i
The %"A, -F!hc pl-t aj~-.,::r r~, us, W",
U"d
w vla nj 1: u2

USSR/Physical Chemistry Thermodynamics. Thermochemistry. Equilibrium. Physico-
chemical,Analysis. Phase Transitions, B-8
Abst Journal: Referat Zhur Xhimiya, No l.. 1957, 380
Author: Tananayev ..Nikolayev, N. S,', Buslayev.. Yu. A.
Inetitution.'m None
Title: Investigation of the System HF-ZrF4-H2O by the Isothermal Solubility
Method (Isotherm 0.50)
Original
Periodical: Zh. neorgan. khimii, 1956, Vol 1, No 2, 274-281
Abstract: The solubility at 0.50 in the system HF-ZrF4_H~10 has been investi-
gated for the range 0-100 percent HF. The following solid phases
were found in the system: ZrOF2-2H2O(I), ZrF4-3H20(II), H2ZrF6'
H20(III), and ZrF4. From thermographic data thermal decomposition
reactions for I, II, III, and ZrOF2 have been established. A method
has been developed for the-determination of both F and Zr when present
together.
Card 1/1

TANAMOZY, I.T.; MARELMISHVILI, N.V.
Study of the formation of silver hydroxide. Zhur.zleorgAhim.
1 no.8:1826-1831 Ag 156. (NLHA 9:11)
(Silver hydroxide)

USSR/Inorganic Chemistry - Complex Compounds. C.
Abs Jour : Ref Zhur - Khimiya, No 9, 1957, 30291
Author : Tananayev, I.V., Seyfer, G.B.
Inst
Title Mixed Ferrocyanides of Magnesium, Rubidium and Cesium
Orig Pub Zh. neorgan. khimii, 1956, 1, No 9, 2017-2023
Abst On the basis of the results of a study of the system
MCI - Mg /-Fe(CH)e 7-H.
.Y- ,0, wherein M is Rb or Cs, by the
solubility method, it was found that the composition of
the solid phase that separates, corresponds to, the for-
mula 3K,&. J. - e(CN),j.l2KO. The composi-
r_Fe(CN) , 4Kg.,L F
tion is not altered on use of an excess of both compo-
nents, in the case of Rb, while in the case of Ce, an ex-
cess of Mg.
- ,-f fe(a)dj causes the formation of
Cs.,L Fe(CN)U.2KgWLFe(CN)47.l0H.3.0.
Card 1/1

-,USSR/Inorganic Chemistry. Complex Compounds. C
'Abs Jour : Ref Zhur - Khimiya, No. 89 1957, 2649o.
Author : Tananayev, I.V., Mzareulishvili, N.V.
Inst : -_
Title Study of Reaction of Zinc Hydroxide Formation.
Orig Pub Zh neorgan. khimli, 1956, 1, No. 10,
22i6 - 2221+.
Abstract The system ZnS(~+ - NaOH - H 0 was studied
by the solubility, the elec?~ical conduc-
tivity, the potentiometric methods and the
methods of light extinction and of precip-
itate volume measurement. It was estab-
lished that the reaction between ZnSO)+ and
NaOH in an aqueous solution proceeds with
the formation first of 4Zn(OH)2,ZnSOI+ M
and of Zn(OH)2 (II) after that. Considering
Card 112

,,TJSSR/Inorganic Chemistry. Complex Compounds. C
Abs Jour Ref Zhur - Khimiya, No. 87 1957, 2649o.
the obtained data, the conclusion was
arrived at that the quantitative determination
of Zn2'~' by titration with an alkali solution
Is possible by the following methods:
a) geometrical (by the formation of I
and II)
b)~ conductometric (by the formation of I),
and
c) potentiometric (by the formation of II).
Card 2/2

T4 at) V *."Y f~' ~': '/ 1; V; .
USSR/Inorganic Chemistry. Complex Compounds. C
Abs Jour Ref Zhur - Khimiya, No. 89 19577 26493.
A
Author Tananayev, I.V., Mzareulishvili, N.V.
Inst
Title Study of Reaction of Cadmium Hydroxide
Formation.
Orig Pub Zh. neorgan. khimii, 1956, 1. No- 10,
2225 - 2231.
Abstract The system CdM - NaOH - H 0 was studied
by the solubil y the elecirical conduc-
tivity, the potenhometric methods and the
methods of light extinction and of precipi-
tate volume measurement. It was established
that the reaction between CdSO)+ and NaOH in
a diluted aqueous solution proceeds with the
formation first of 4Cd(OH)2-CdSN and of
Card 1/2

USSR/Inorganic Chemistry. Complex Compounds. C
Abs Jour Ref Zhur - Khimiya, No. 81 19579 26493.
1
Cd(OH)2 after that. Considering the ob-
tained data, the conclusion was arrived at
that the method of light extinction is appli-
cable to the quantitative determination of
Cd '~_ by titration with an alkali solution.
Card 2/2

TANANAYEV, I.V.; ULIYANOV, A.I.
Physicochemleml analysis of systems important in analytical chqmistry.
Part 25. Study of the caprocIpitation of alkali metal sulfittes vIth
BaSO4. Trudy Kem.an^l.khIm. 7:3-20 '56 . (MLRA 9:9)
I.Institut obahch4v I nearganichoskoy khtaii insul. N.S.KurnRkova AN
SSSR. (Sulfates)

TANANAYEV, 1. V.
"The possibility of separating francium from cosium.9
report presented at The Use or Radioactive Isotopes in Analytical
Chemistry. Conference in Moscow, 2-4 Doe 1957
--- MR. 1958. No. 2. (&uthor Rodin. S. S.)

TANARATIT. I.T.j LITITA, N.I.
Nood"lum forroclaalde*. Xhia.refteelose no*3:28-0 157o
(MLRA 10:8)
I.Inatitut obehohey i neorganichasker Wall in. N.5. gurnakova
Akad sli nark SSSR.
(Noodystum forrqcyanldoo)

137-58-2-4398
Translation from: Referativnyy zhurnal, Metallurgiya, 1958, Nr 2, p 300 (USSR)
AUTHORS: Tananayev, 1. V, Bausova, N.V.
TITLE: Gallium Ferrocyanides and Their Analytical Significance (For-
rotsianidy galliya i ikh analiticheskoye znacheniye)
PERIODICAL: Khimiya redkikh elementov, Nr 3, 1957, pp 41-56
ABSTRACT: Tests of solubility, light absorption, electrical conductivity,
and e. m. f. were used to study the reaction 'of Ga, ions with~ the
ferrocyanides of Li, K, and Na. Iry all the systems studied it
was found that Ga 4 [ Fe(CN)61 3 forms. Whenever surplus K4
[ Fe(CN)61 and Na4 (Fe(CN)61 were present, formation was
observed of mixed salts of NaGa [ Fe(CN)61 (the HZO dissociat-
ing) and KGa [Fe(CN)6 j (soluble congruently). On the basis of
the data obtained, new methods are proposed for determining
Ga. Potentiometric titration with an Na4 [Fe(CN)61 solution
made Possible the determination of Ga in the presence of an Al
content 100 times greater. With Na4 [ Fe(CN)6 I in a 100-cc
solution it was possible to determine 0.2-30 mg of Ga by means
/Z of the heterodyne method. Amperometric titration with a K4
Card I [ Fe(CN)6 I solution could be carried out in the presence of

137-58-2-4398
Gallium Ferrocyanides and Their Analytical Significance
large quantities of Al, since the presence of the Al was reflected only in the
slope of the titration curve.
N.G.
1. GalUm forrocyanUes-Analysis
Ca rd 2/2

-7;~&,9=j~;~rvl P'll,
N, R.N.; un"TIT. I.T.
40-6#~
Study of the reaction of indi= hydroxide forvatl*v. Kbisiveft.
ales. no.3:73-86 '37. (nu 10:8)
Llustitut obsbaboy I nearganicheskoy Wall In. N.S. Kuruskove
Akmdsull nauk SSSR-
(Indium hydroxideO

1. ~- ~ ~ ~- -7- . ~ -~ -:., ~~ ~ -- II . I' . .- . . I.--- -.-
I i
1. .- l M i IBM 4
. -~ ~ M Em.
lowm9mvp-i M~-- I-V iMEMAM
mse4m. sm~

AUTHOR- -I!=-!N ~~IIVZ 62-12-1/20
TITLE: New Data Concerning the Chemistry of Some Rare Elements (Novyye
dannyye o khImii nekotor7kh redkikh elementov)
Lecture Delivered at the Meeting of the Department of Chemical
Sciences of the AN USSR on October 31, 1957 (Doklad na, sessii
otdeleniya khimichaskikh nauk Ucademii nauk SSSR 31 oktyabrya
19579).
PMODICALt Izvestiya AN SSSR Otdolen%e Khimicheakikh Nauk, 1957, Ur 12,
Pp. 1421-1428 (USSR)
ABSTRACTz Among the questions of greatest interest at present in physical cherr-
Istry there is also that of the elaboration of now reactions of rare
alkaline metals. Nearly all of them form practically Unsoluble raixed
ferrocyanides Ath alkaline metals (see table 1). Wm solving the
problem concerning easier methods for the production of a partiou-
larl,y pure liquid fluorine hydrogen and fluorine, the fluorine com-
pounds of lithium, zubiaium and cesium vin attain particular im-
portance. The lecture contains new data concerning the composition
and the physical properties of various compounds of some rare ele-
ments. Among other tbings, also a survey is given of the insoluble
Care 1/2 mixed ferrocyanides, camposed of various metals with lithium,

New Data Concerning the Chemistry of Some Rare Elements. 62-1, 2-1120
Lecture Delivered at the Keeting of the Department of Chemical
Sciences of the AN USSR on October 31, 1957'
rubidium and cesium. In this connection the lecturer recommends a
number of now reagent precipitations. A rule governing the modifi-
cation of the composition of mixed ferrocvanides containing rare
a3laline earth metals ~ms determined. Further, new details are
given concerning the compositicn ana aurability of fluorides, oxa-
lates, tartrates, and other compounds of gallium, indium, zirconium
and germanium. There are 2 tables.
ASSOCIATICK: Institute for General eM Inorganic Chemistry imeni H.S.Kurnakov
AN USSR (Institut obshchey i neorganicheskoy khimii im.
N.S.Kurnakova Akaaemii nauk SSSR).
SUBMITTED: October 9, 1957
AVAILABLE: Library of Congress
Card 2/2 1. Chemical engineering-Conference 2. Flourine-Liquid
3. Flourine Wrogen-Liquid 4. Lithium 5. Rubium

AmIlOR: Tananaev, I'.V., Seifer, G.B.9 and Glusbkovat M.A. 560
Tit=: Ferrocyanides of Trivalent Iron (0 Ferrotsianidakh T-rekhvalent-
novo Zheleza.)
PERIODICAL: "Zhurnal Neorganicheskoy Khimii", (Journal of Inorganic Chemistry
Vol,II, No'.29 pp.268-280. (U.S.S.R.) t,(s-7
ABSTRACT: In this investigation the behaviour of the cyanides of trivalent
iron in systems with lithium? sodiump potassiumt rabidium and
caesium has
b.een studied by two methods: that of solubility and
.
that of e m.f. measurement. The equilibrium solutions obtained
in the solubility experiments were used for the parallel study o
the systems by the e.m.f. method using a platinum electrode with
a saturated calomel electrode-,; From the results obtained conclu
sions are drawn on the general'behaviour of trivalent iron ions
in and ferrocyanides of different alkali metals when present to-
gether in systems. Differences due to the nature of the individ
ual alkali metals were also noted. The tendencyl to all the alk
1i metals was the formation of mixed ferrocyanides of iron al-
though the nature of these compounds was very different for the
different alkali tal The-stoichiometrically normal iron
ferrocyanide Fe4X(Cn%J3 is not formed with any of the systemE
studied. On incomplete precipitation of iron it ith r becomes
j e e
adsorbed (systems with Li4[Fe (0n)6],, and Na4 [Fe On) 611 ), or remaJ
Card 1/2

Ferrocyanides of Trivalent Iron (Cont.)
560
in excess (systems with K4 (Bb Cs4)[ke(Cn)61 ), an effect evident-
ly due to coprecipitation of thle alkali met&l.
N(On)61
Card 2/2
enters the precipitate as soon as the precipitat-
M4
ion of-iron is comDlete even with lithium and sodiud. This is
~9'jj]
composition M6Fe2 Tie
6-13-
Although the continued adsorption of X4[Fe(Cn)g] by the
precipitate makes the interpretation of thd experiffiental curves
difficult the possibility of the formation of new incongruently
soluble mixed salts of definite composition is not excluded.
especially pronounced with rubidium and caesium. The contents of
alkali metal in tile precipitate increased according to the series
K - Rb - Cs.
It appears that with potassium, rubidium and caesium mixed
salts of the simplest type M FeTe LCn)K1 are formed at first. It
is very likely that the salts; 1E1bFeLFe(On) :land CsFe rle(Cn)G~ do
to form a second
existp but they react easily with M4 [Fe
mixed salt of the
Ch
ferrocyanides
inorganic prototypes of ion-exchange resins.
As regards the strength of the bond in mixed ferrocyanides of
iron and alkali metalsy the latter can be arranged in the usual
series with caesium having the greater strength and lithium the
least. Apparently in the mixed salts the alkali metals can mutual
replace each other according to the above order'. From this point
view mixed
of trivalent iron can be considered as
14 Figures and 5 Tables.

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Card 1/2
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t1aa
561
Mixed Ferrocyanides of Thalli-Um. I. Mixed Ferrocyan des of
"hallium with magnesium, Calcium and Strontium (Cont.)
resembij them: this is indicate b
'y the fact that they all
belong io the single type 112E Fe (CN) ] ' As regards solu-
bility in water, the Compounds of tWi'i~m considered most
closely resemble the corresponding rubidium and caesium
compounds.
There are 3 figures and 3 tables.
Received on 22nd October, 1956.
Mere are 7 referencesp one of them Russian.
Card 2/2

-T
,O~-N
AUTHORS: Tananayev, I, V. and Levina, M. 1. 78-3-12/35
TITLE: Some Data on the Structure of Mixed Ferrocyanides.
(Nekotoryr dannyp o strqenii smeshannykh ferrotsianidov).
PERIODICAL: Zhurnal Neorpnicheskoy Xhimii, 1957, Vol.II, Nr.3,
pp.'576-585. (USSR)
ABSTRAGT: The addition of silver nitrate to an aqueous suspension
of any mixed forrocyanide leads to the displacement by
the silver ions of both cations of the mixed salt from
the precipitate into the solution. If the silver
nitrate is added gradually and the concentration of the
cations of the mixed salt in the solution is determined
on each addition, the order and degree of replacement of
the heavy and alkali metals of the mixed salt by silver
can be found. This is the basis of the method used in
the present investigation, except that the process was
followed by determining the silver concentration in the
su ernatent liquid by measuring its radioactivity.
AgYlO was used as the tracer. The following compounds
Card 1/2 were studied: X4Ni4[F8(CN)6]3 and

78-3-12/35
Some Data on the Structure of Mixed Ferrocyanides.
5G02[Fe (CN) 6] X4 LFe (GN) jand also N12[Fe(GN)J.
The method used enabled the relative strength of the
bonds of the metals in the outer sphere of mixed
ferrocyanides with ferrocyanide ions to be found, and
it is suggested that this should influence the way in
which the chemical formulae of metal mixed ferrocyanides
should be written. Based on a study of the conditions
for the formation of KAg [Fe(GN)61 analytical methods
are recommended for the determination of small quantities
of silver and ferroeyanide in solutions radiometrically
with the use of Ag1lO and also potentiometrically.
There are 7 figures, 13 tables, and 11 references, a of
which are Slavic.
SUBMITTED: October 27, 1956.
AVAILABLE: Library QfCongress.
Card 2/2

78-3-13/35
AUTHORS: Tananayev, I* V. and Glushkova, M. A*
-TITLE: Mixed Ferrocyanides of Thallium. (0 smeshannykh
ferrotsianidakh talliya.) II. Mixed Ferrocyanides of
Thallium with Copper and Nickel. (II. Smeshannyye
ferrotsianidy talliya s medlyu i nikelem.)
PERIODICAL: Zhurnal Neor anicheakoy Xhimil,, 1957, Vol.II, Nr.3.,
pp. 586-593. fUS3R)
ABSTRACT: This Investigation had as its aim to fill the gap In
the literature on the nature of the reaction of copper
and nickel ions with ferrocyanide ions in the presence
of thallium.. The potential importance of such an
investigation is that the information it provided will
be used to decide whether thallium in very low con-
centration could be isolated from solutions containing
certain non-ferrous metal:s. Ordinary methods of
chemical analysis were used in thifi investigation to
study systems ensisting of Ti*p 34* (E = Gu, Ni)
and [Fe(CN)6] . It is concluded that thu slightly
Card 1/2 soluble mixed ferroeyanide of thallium and copper,

Mixed Ferrocyanides of Thallium. II.
78-3-13/35
T12CU2[Fe(CN)612, is formed from the appropriate ions
for the whole range of concentrations dealt with. The
solubility of the Rompound formed as a result of the
displacement of Gu4'~'ions by Tl* ions from a precipitate
Of Cu2[Fe(CN)6] was found to be so small that a suspension
of this precipitate can be used to separate small
quantities of thallium, from solution. The mixed nit
T14N14[F6(GN)613 was formed by the reaction of Ti
with N12+ and [Fe(CN) 4- Ions.. T.ho.solubility of !~90
precipitate of this sqat, formea by 'tile reaction of TI
Ions with a precipitate of nickel ferrocyanide is so low
that it, too, can be used for separating small quantities
of thallium from solution. There are 4 figures, 7
tables, and 6 references 2 of which are Slavic..
SUBMITTED: October 26, 1956.
AVAILABLE: Library of Congress.
Card 2/2

V _7-
78-3-14/35
AUTHORS: Tananayev, 1. V. and Glushkova, M, A,
TITLE: FerrocyanideB of Thallium. (0 Ferrotsianidakh
talliya.) III. Mixed fGrrocyanides of thallium with
uranyl. (III. SmesharrWye ferrotsianidy talliya s
uranilom.)
PERIODICAL: Zhurnal Neorganicheskoy.Khimii, 1957, Vol.I1, Nr*3,
pp. 594-599. (USSR)
ABSTRACT: An account is given of the study of the solubility of
the system TM~902(N03)2 _L14D?G(GN)61-H2O at 25'G.
Solutions of these compounds were used, the molarity of
the thallium nitrate solution being determined by
precipitating thallium as chromate, that of lithium
cyanide by titration of a known volume of the original
solution by potassium manganate in sulphuric acid
using crystal violet as an indicator. The concentration
of thuiranium salt was determined by precipitation of
(U02)2 in the presence of carbonate-free ammonium
nitrate, the precipitate after washing and calcining
Gard 1/2 being weighed as U3% . No formation waS of

F;rrocyanides of Thallium. 111.
78-3-14/35
the simple ferrocyanide of uranyl, the reaction of the
ions leading to the formation of two mixed ferrocyanides
of thallium. and uranium with the compositions:
T12(UO2)3[Fe(GN)612 and T14(U02)4[Fe(CN)6]3. All the
alkaline metals and thallium can be arranged in the
following series with respect to their ability to
displace [U02324' ions from the precipitate of
(U02)2 [Fe(ON)61 : T1 is jX Go > Rb >P K > Na >, Li,
from which it follows that suspensions of this precipitate
can be used for separating small quantities of thallium.
from solution. There-are 2 figures, 6 tables, and 5
references 2 of which are Slavic.
SUBMITTED: November 19, 1956.
AVAIIABLE: Library of Congress.
Gard 2/2

-T-A
AUTHORS: Tananayev, I. V. and Seyfer, G. B.
TITLE: Mixed Ferrocyanides of Calcium with Rubidium and
Caesium. (Osmeshannykh forrotsianidakh kalltsiya
a rubidiyem i teeziyam.)
PERIODICAL: Zhurnal Neor anicheskoy Xhimii, 1957, Vol.II, Nr.3,
pp, 600-603. fUSSR)
ABSTRACT: All methods previously proposed for utilizing the
reaction of the formation of mixed calcium ferrocyanides
have lacked a proper experimental foundation, and thua
lead only to qualitative results. The provision of
experimental data sufficiently accurate and full to
enable quantitative results to be obtained is the object
of the present investigation. Solubilit ethods were
used to study the systems in the MC1- Ca2 9(CN)6]-H20,
where N - Rb'O' or Gs+, which enabled the influence of
excess of the components on the composition of the
compound formed to be followed. The experimental
method used has been previously described7. For the
Card...1/3 rubidium system it was found that the ratio of

Mixed Ferroeyanides of Calcium with Rubidium and Caesium. 78-3-15/35
[pe(cN)614- : Rb+ and of [Fe(CN)6]4- : Ga2+ do not
depend on the ratio of either component in the mixture,
that is the precipitate obtained is constant in
composition. The mixed ferrocyanide obtained is
represented by the formula Rb2()R[Fe(CN)6]. Similar
results were obtained for the caesium system, the
precipitate here being 0320a[Fe(CN)6]. Although results
obtained suggested that the formation of the mixed
ferrocyanides of calcium could be used for the gravi-
metric determination of rubidium. and caesium, it was
found that this could only be done with perfectly pure,
solutions, since the solubility of the precipitates
formed is very strongly affected by the ionic strength
of the solution; further, the small difference in the
solubilities of the rubidium and caeaium salts makes it
unlikely that the reaction could be used for separating
rubldium and caesium. There are 2 figures, 2 tables,
Gard 2/3 and 8 references 2 of which are Slavic.

Mixed Ferroeyanides of Calcium with Rubidium and Caesium.
ASSOCIATION: Institute of General and Inorganic Chemistry imeni
N. a. Kurnakov;. of the Academy of Sciences of the USSR.
(Institut obahchey.ineorganichesko-y khimii im. N.8,
Kurnakova AN 383 R.)
SUBMITTEDs October 27, 1956.
AVATr.Agj&: Library of Congress.
Card 3/3

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- - - ---------------------
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BWFhY8lc&l
Abs jo,,r, &Mrna- Solutifts' Theory Of A,144
&tMjYvL ' 'V0 2, 1958, 3945. and Bases.
Olu I 80-lut:Ecms and Al(
e. 2
f Al in Presezice Of 203) solutlons Can be used fOr deterldnaticm
Card
2/2

TARARAM, I.Y.: VINOGRADOVA. A.D.
, -
Gompo-sition and stability of fluoRluminates in solutions. Zhur.
neorg. khim. 2 10:2415-2467 0 157. (MIRA 11:3)
(Fluoaluminates) (Solution (Chemistryv

TANAMAYEV,,I.V.-, IONOTA, Ye.A.
Zirconium forrocyanides. Part 1: Interaction of ZrOC12 with
11&41]Pe(CN)61 and %[J'~(CN)�1 in aqueous solutions. Zhur. neorg.
khtm'. 2 10:2468-2474 0 57. (MIRA 11-3)
1. Institut obahchey i neorganicheekoy khimil Im. N-S.Kurnakova
AN SSSR.
(Zirconium compounds) (Sodium ferrocynnide)
(Potassium forrocynnide)

TANANAM. 1. V. -. OWSHIODVA, N.A.
Thallium forrocynnides. Part 4: Mixed forrocynnides of tbpklliuo
with lanthanum and cerium. Zhur. neorg. khis. 2 lo:z474-2482
0 157. (MIU 11:3)
(Thallium ferrocynnide) (Lanthanum) (Cerium)

TANANA I LIBOOMLIDAR, M.Ya.
Investigating the formation of nickel hydroxide In aqueous solutions.
Zhur, neorg, kh1n, 2 no.12.-2700-2706 D '57. (MIRA-11:2)
1, Hoskovskly inzbenerno-fizicheekly Institut, Rafedra, khimit.
(Nickel hydroxide)

jC~19NAL OF ANILYTICAl. CF,-t,%GSTRY
vc"~ U1, Nr 4, 19517
.11 fusutuw

AUTFORS; Tananayev, I. V., Shcheglova, Ye. P. 75-6-11-23
TITLE. Investigationer of the System BeSO 112OH-H 0 and its Ana2v-ticz-l
4-~ 2
Application (Issledovaniye sistemY, BeSOeaOH'420 ' yeye ara]'i U-
cheskoye primeneniye).
PERIODICAL: Zhurnal Analiticheskoy Khimii, 1957, Vol- 12, 'Nr 6, pp. 671-676
(USSR).*
ABSTRACT! The solubility in the system BeSO 47 11aOH-H.O at 250C was irr-restiga=
ted. It was stated hereby that with the formation of Be(OH)2 firstj
szoluble basic salt-T, are fermed and then follows the forma-V-ion of
insoluble basic salts of variable composition. Beryllium hyd-~oxide
dissolves in alkaline lye-solution when the content of alkaline lyE
attains 0,025 mol. per liter. A combined alkali-oxy-quinolate r.',ethoe
is preferred for the determination of beryllium in the presence of
larger quantities of aluminum. The complete separation of beryllilr
and alirninum. on the strength of the different solubility of their
hydroxides in alkaline lyes does not lead to a quantitative separa-
tion.of aluminum and beryllium.
There are 1 figure, 3 tables., and 8 references, 4 of which are Sla-*
Card 4/2 VIC.

Investigations of the System BeSO 4-'TaOff-H2 0 and its Analytical 75-6--1/2.17
Application.
ASSOCIATION: Mosew Institute or Engineiering Physics (Moskmkiy
inshenern6-fizicheekiyIinatitui).
SUBMITTED: January 4, 19-iZ-.,
AVAILABLE: Library of Congress.
1. Chemistry-USSR 2. Beryllium hydroxide-Solubility
3. Alkaline lye solution-Applications 4. Aluminum-Beryllium
content-Determination
Card 2/2

5W
AUTHORSt Vasil*yev, V. P., Korableva, V. D.p SOV/153-58-3-30/30
Yatsimirskiy, K. B.
TITLEs Conference Discussion on the Methods of Investigating the
Complex Formation in Solutions (Boveshohaniye-diskussiya
po metodam izueheniya komplaksoobrazoveniya Y rastyorakh)
PERIODICALt Izvestiya vysshikh uohobnykh zavedeniy. Xhimiya i
khimiohaskaya t*khnologiys,, 1958, Nr 3, PP 173 - 174 (USSR)
ABSTRACTs From February 18 to 21, 195E1 a conference discussion took
place at the town of Ivanovo; it dealt with the subjects
mentioned in the title. It was called on a decision of the
VIIth All-Union Conference on the Chemistry of Complex
Formations. More than 200 persons attended the conference,
among them 103 delegates from various towns of the USSR.
At the conference methods of determining the composition of
the complexes in solutions were discussed, as well as the
methods of calculating the instability constants according
to experimental data and problems concerning the influence
of the solvent upon the processes of complex formation.
I. I. Chernyayev, Member, Academy of Sciences, USSR, stressed
Card 1/16 in his inaugural lecture the great importance and actuality

Conference Discussion on the Methods of SOV/153-58-3-30/30
Investigating the Complex Formation in Solutions
of the problems to be dealt with, and wished the conference
all the best in its work. I. V. Tananayev, on behalf of the
Orgkomitet (organization Committee) held a lecture on: "The
Method of Determining the Composition of Compounds Formed in
Solutions". In his lecture, V. N# Tolmachev dealt with the
problem of the graphical interpretation of the method by
Ostromyslenskiy-Zhob. It was proved that this method can
also be used in such cases where the equilibrium of complex
formation was turned complex by the hydrolysis or dimerization
of the central ion. In the lecture by L. K. Babko and
M. M. Tananayko, "Physical and Chemical Inslysis of the
Systems With 3 Colored Complexes in the Solution", the results
of a systematic investigation in copper-quinoline-salicylate,
as well as in copper-pyridine-salioylate systems by means of
the optical method were dealt with. In the lecture by Ya. A.
Fialkov the idea of a further investigation of the complex
formation processes in solutions was developed. Besides the
determination of the composition and stability of the complexei
also the physical and chemical properties, the chemical nature
Card 2/16 and the structure of the complex compounds must be investi-

Conference Discussion on the Methods of BOV/153-58-3-30/30
Investigating the Complex Formatio.n in Solutions
gated. The lecture by K. B. Yatsimirsk dealt with the
conditions of checking the usefulness of the method of iaomolar
series in the determination of the complex composition. To
be able to obtain objective results the position of the
maximum at various concentrations of the components must be
checked. A. K. Babko made several critical remarks concerning
the lecture by I. V. Tananayev. He pointed out that such a
method of investigation must be chosen that is connected with
the characteriatic'propertiee of the system investigated.
A. F. Komar' mentioned in his lecture that for the time being
the method by Ostromyslenakiy-Zhob is the best for determining
the complex composition, and should be employed as often as
possible. This demands, however, that all instructions con-
cerning this method are strictly obeyed. I. S. Rustafin,
L. P. Adamovich and V. I. Kuznetsov took part in the discus-
aion. K. B. Yatsimirskiy proved in his lecture "Hydrolytic
EquilibFfa an the Polymerization in Solutions" that, if the
hydrolysis products are polymerized, the "inclusion into the
complex" and the "formation function" at a constant pH value
Card 3/16 are varied with the modification of the total concentration of

Conference Discussion on the Methods of SOV/153-58-3-30/30
Investigating the Complex Formation in Solutions
the metal. Therefore all those methods may be employed for
investigating the polymerization of this type which make the
determination of at least one of the two functions mentioned
possible. It was proved that the hypotheses on the existence
of complexes of the type "nucleus + chain members" can also
be founded from the viewpoint of structural concepts: psrticle~
the charge of which does not exceed unity can occur as "chain
members". The usefulness of the characterization of areas of
existence of pdymers by means of surface diagramss "total
concentration of the metal - pH11 was proved as well. I. I.
Alekseyeva and K. B. Yatsimirskiy in their lecture "Investiga-
tion of the Polymerization of Iso-Poly Acids in Solutions"
mentioned experimental results of the investigation of the
polymerization in solutions of molybdic acid. The authors
proved that especially the molybdic acid within a certain
range of the pH values and the concentrations exists as a
number of compounds that can be expressed by an overall formul
goo4(HMOO4)n-2. In the lecture by N. V. Aksel'rud and V. B.
Card 4/16 Spivakovskiy investigation results on basic salts taking into

Conference Discussion on the Methods of SOY/153-58-3-30/30
Investigating the Complex Formation in Solutions
account the complex formation in solutions by means of the
potentiometric method were mentioned for systems with zinc,
cadmium and indium. In the evaluation of their results the
authors employed the method of the table difference. The
calculation of the consecutive constants was carried out
according to the interpolation formula by Newton. M. A.
Chepelevtskiy held a lecture on "pH Measurement Method of
the Solutions in Combination With t~q System Analysis of the
Solubility Diagram of the System Cu~MHCl - H2 0 in Investiga-
ting-Complex Copper Compounds in Saturated Solutions". It
was found that the substance at the bottom of the liquid is
more basic than the solutions furthermore, the increased
acidity of the solution from the viewpoint of the formation
of hydroxy-ohloro complexes in the solution'w" explained.
V. r. Kuznetsov opened the discussion with his lecture; he
pointed 'but'the necessity of utilizing the concepts worked
out in the investigations of the polymerization in organic
chemistry in the chemistry of polynuclear complexes. A. A.
Card 5/16 Grinberg thinks that the new approach of the hydrolysis

Conference Discussion on the Methods of SOV/153-58-3-30/30
Investigating the Complex Formation in Solutions
investigation as developed by the Scandinavian school is of
high value. He also pointed to the necessity of studying
the kinetics of the polymerization process and a quantitative
determination of the strength of the polymers. A. K. Babko
pointed out that the study of the polymer structure was
necessary. N. P. K~mar' mentioned in his lecture that the
rather widely spread polymerization type according to the
scheme "nucleus + chain members" is not obtained in all casei
The following scientists took part in the discusBions V. N.
Tolmaohev, A. V. Abloy, 1. S. Mustafin, I. V. Tananayev and
K. B. Yataimirskiy. A. K. Babko then discussed in his lecturo
"Methods of Determining the Dissociation Constant of the
Complex Groups in Solutions" the main principles of determini
the instability constants. N. P. Komar' discussed in his
lecture "Calculation Methods of the Instability Constants of
the Complex Compounds According to Experimental Data" the
possibilities of using the known calculation methods of the
instability constants for various cases of the complex forma-
tion in solution. If *several mononiiolear complexes are f orm,
Card 6/16 the displacement method by Abegg and Bodlender (completed by

Conference Discussion on the Methods of SOV/153-58-3-30/30
Investigating the Complex Formation in Solutions
1. K. Babko) cannot be recommended for the calculation of
the instability constant. The leoturer discussed the dis-
solution methods of the polynomials proposed by B'yerrum,
Leden, Rossoti, Sketchard, Edsolloy and other authors. The
constants calculated in this way are not very accurate. It
was proved that the method of successive approximations can
lead to wrong conclusions as to the chemical processes taking
place in the system investigated. The most probable value
of the physical constants can be obtained by the method of
the least squares. B. V. Ptitsyn, Ye. N. Tekster and L. 1.
Vinogradova described the determination methods of the
instability constants of the -oxalate complexes of niobium,
uranium and iron which are based on the investigation of the
equilibrium displacement of the complex formation by silver
ions. N. X. Bol'shakova, I. V. Tananayev and G. S. Savch6nko
held'a lecture on "The Role of the Time Factor in the Investij
tion of the Complex Formation". In the discussion on the
lectures A. A. Grinberg mentioned that due to the slow
adjustment of the equilibria the methods discussed of
Card 7/16 determining the instability constants (palladium and cobalt

Conference Discussion on the Methods of SOY/153-58-3-30/30
Investigating the Complex Formation in Solutions
complexes) can often not be employed. A. V. Ablov pointed
out the necessity of devising direct methods of proving the
existence of intermediate forms in a step-wise complex forma-
tion. K. B. Yatsimirskiy mentioned that the instability
constants of slowly dissociating complexes can be calculated
from thermochemical data. L. P. Adamovich, A. V. Golub
among others took part in the discussion on the lectures.
A. K. Babko requested inclusion in the next conference on the
chemistry of complex compounds a lecture in which various
calculation methods of the instability constants should be
discussed by the example of actual cases. This should clarify
to which divergencies of the values of the constants dif-
ferent methods of evaluating the experimental data can lead.
N. P. Komar' stressed that in the determination of the
instability (.onstants all chemical equilibria should be taken
into account that render complex the complex formation process
in the solution, especially the hydrolysis processes of the
central ion and the addendum. In the lecture delivered by
V. U. Peshkova and A. P. Zozulya "Application of the Distribu-
Card 6/16 tion Method to the Investigation of the Stability Constant's

Conference Discussion on the Methods of SOV/153-58-3-.30/30
Investigating the Complex Formation in Solutions
of Some Thorium Complex Compounds" results obtained from the
experimental investigation of the distribution of thorium
compounds in the systems: acetylacetone benzene - water, and
2-oxy-1,4,-naphthoquinone - chloroform water were given.
From these data the instability constants of the thorium
complexes with acetyl-acatone and 2-oxy-1,4-naphthoquinone
were calculated. I. V. Tananayev, 0. S. Savchenko and Ye. V.
Goncharov held a lecture on the application of the solubility
method in the determination of the stability of complex
compounds in solutions. In this lecture also other methods
of investigating complex formation processes in the solution
were discussed (pH measurement, measurement of the optical
density, as well as of the heat of mixing). B. D. Berezin
held a lecture on the "Application of the Solubility Method
in Studying the Phthaloeyan~kne,Complexes of Metals". He
used the determined quantitative characteristics of the
reaction of the transition of the phthalocyanides of cobalt,
nickel, copper and zinc, as well as of the free phthalo-
oyanine into the sulfuric acid solution for the theoretical
Card 9/16 reasoning, and as an experimental proof of the existence of

Conference Discussion on the Methods of SOY/153-58-3-30/30
Investigating the Complex Formation in Solutions
~f-bonds in the complexes investigated. These characteristics
also served him as a proof of new electronic formulae of
phthalocyanine and its complex derivatives. In the lecture
delivered by I. L. Krupatkin on "The Method of the Two Solventi
as a Method of Investigating the Formation and Properties of
Organic Complexes" it was proved that this method makes it
possible to determine the number of complexes formed in the
system, their composition and relative stability. V. I.
Kuznetsov, A. K. Babko, N. P. Komar', I. S. Mustafin and
Ya. I. Tur'yan took part in this discussion. In the lecture
delivered by A. A. Grinberg and S. P. Kiseleva on the complex
palladium compounds (II) with a coordination number above
four it was proved that in the case of a farge chlorine and
bromine ion excess complexes with the coordination number 5
are formed. The instability constants of these complexes
were estimated. L. P. Adamovich mentioned a new manipulation
in the spectrophotometric investigation of the complex com-
pounds that can be used in systems with the formation (or
predomination) of one single complex. This method makes it
Card 10/16' possible to determine the composition and instability constan,

Conference Discussion on the Methods of SOY/153-58-3-30/30
Investigating the Complex Formation in Solutions
of the complex. In the lecture delivered by K. B. Yatsimirskiy
and V. D. Korableva the application of the theory of crystal-
line fields for the determination of the composition and
structure of the chloride complexes of cobalt, nickel and
copper according to the absorption spectra of these complexes
was discussed. It was proved that in a hydrochloric acid
concentration above 5 mole/liter in the solution there exists
an equilibrium between the tetrahedric and octahedric form
of the cobalt chloro complexes. Yu. P. Nazarenko proved in
his lecture "The Application of Radioactive Isotopes in the
Investigation of the Solvation Equilibrium in Solutions of
Complex Compounds" the possibility of using data on the
isotope exchange to clarify the structure of the complex and
mechanism of the hydration processes. V. Klimov mentioned
in his lecture the use of radioactive isotopes in the study
of tin and antimony oomplexes in non-aqueous solutions. A. V.
Ablov, V. N. Tolmachev, V. I. Kuznetsov and A. 1. Golub took
part in the discussion of the lectures. The usefulness of
employing the theory of the crystalline fields in explaining
Card 11/16 the results obtained from the absorption spectra of the com-

Conference Discussion on the Methods of SOY/153-58-3-30/30
Investigating the Complex Formation in Solutions
plex compounds was stressed. In the lecture delivered by
I. A. Shek on "The Investigation of the Complex Formation
by the Method of the Dielectric Permeability and the Polariza-
tion" the principles of the methods mentioned were presented.
This method was employed for investigating the compounds of
the type of the "affiliation" products. The lecture delivered
by I. A. Shek and Ye. Ye. Kriss "Employing the Method of the
Dielectric Constant for Investigating Complex Compounds of
the Type of Crystal Solvates in Solutions"-dealt with the
investigation of the solvates of lanthanum and cerium chlorides
with ketones, as well as with the study of the compounds
formed in heterogeneous systems with tributyl phosphate and
nitric acid. V. F. Toropovs. gave in her lecture "The Polaro-
graphic Method of Investigating the Complex Formation in
Solutions" a survey of the applications of the polarographic
method in the study of the complex compounds, and illustrated
several fine characteristic features of this method. In the
lecture delivered by T. N. Sumarokova "The Cryoscopic Method
of Investigating the Complex Formation Reactions" a survey of
Card 12/16 the possibilities of the cryoscopic method was given, and its

GoAference Discussion on the Methods of SOY/153-58-3.-30/30
In7eatigating the Complex Formation in Solutions
applicability in the study of several complex compounds of
stannic chloride with organic substances was proved. A. X.
Golub described the results of his investigations of thio-
cyanate complexes of several metals. A vivid discussion took
place on the lectures hold. Y&. A. Fialkov. and Yu. Ya.
Fialkoy considered the cryoscopic method of investigating
complex compounds to be of considerable value. K. B.
Yatsimirskiy pointed out that the publication of the surveys
on individual methods of investigating the complex formation
reactions would be desired; this concerns especially the
polarographic method. The oryoscopio method should be brought
to a level that makes the calculation of the equilibrium
constants of the processes to be investigated possible. The
problem of the method of evaluating the.oxperimental results
becomes more and more important. Many scientists use the
instability constants without taking into account the way
in which they had been obtained. The calculation methods
employed by 1. M. Golub are one stop back, as compared to
those employed at present. In his lecture N. P. Komar'
Card 13/16 pointed out the extremely great importance of the mathematical

Conference Discussion on the Methods of SOY/153-58-3-30/30
Investigating the Complex Formation in Solutions
evaluation of the results obtained, as well as of the plotting
of-curves. 1. K. Babko suggested belecting one or two systems
that are experimentally well investigated, and to evaluate
the results obtained according to different methods so that
it in possible to check and evaluate them. Ya. 1. Tur'yan
took part in the discussion. Ya. A. Fialkoy discussed in
his lecture "The Effect of the Solvent on the Complex Formation
Process as Vell as on the State of Equilibrium in the Solutions
of Complex Compounds" the influence exerted by the solvents
upon the molecular state, upon the solvation of the system
components, upon the stabilization of the complexes formed
in the system, upon the step-wise dissociation of the complexes
and upon a number of other processes. The influence exercised
by the dielectric constant upon the complex formation process
was discussed. It was concluded that a direct relation does
not exist, and that the chemical nature of the solvent must
be taken into account. A. V. Abloy and L. V. Nazarova held
a lecture on "The Spectroscopic Investigation of Nickel Cobalt
'Pyridinates' in Various Solvents". The instability constants
Card 14/16 of the complexes were determined and it was proved that the

Conference Discussion on the Methods of SOV/153-58-3-30/30
Investigating the Complex Formation in Solutions
stability of the lpyridinates' is changed in dependence on
the solvent. Y&. I. Tur'yan in his lecture "The Influence
of the Bolvent Upon the Composition and Stability of Complex
Ions" discussed the polarographic investigation method of
the chloride and thiocyanate complexes of lead in aqueous
ethanol solutions at different content of the non-aqueous
solvent and at a constant ionic strength. A step-wise
character of the complex formation was found as well as the
instability constants of the complexes. The influence of
the dielectric constant of the solution on the stability of
the investifated complexes was proved. In the lecture by
V. P. Vasil yev on the "Investigation of Aquo Complexes in
Mixed Solvents" the main attention was devoted to the neces-
sity, of the qualitative recording of the dolvation effects
in the complex formation. The applicability of the pol&ro-
graphic method in the determination of the composition and
stability of the &quo complexes in mixed solvents was proved
and experimental material on the thermodynamics of the
dissociation of the cadmium-aquo complexes in aqueous ethanol
Card 15116 solutions was mentioned. V. N. Tolmachey, V. 1. Kuznetsov

Conference Discussion on the Methods of sov/153-58-3-30/30
Investigating the Complex Formation in Solutions
and I. V. Tananayev stressed in their lectures the necessity
of a more complete and general investigation of the solvation
processes. 1. K. Babko and A. M. Golub pointed out the
great importance of the investigations of the complex forma-
tion equilibria in non-aqueous solutions, and made several
critical comments on the lecture-by Ya. 1. Tur"yan. The
following scientists took part in this discussioni L. P.
Adamovich, 0. 1. Khotayanovskiy, A. P. Moskvin and A. G.
Mustakhoy. At the final meeting of the~conference A. A.
Grinberg, Corresponding Member, AS TISSR, said in his speech
that such a conference was very urgent. A detailed discus-
sion of the determination methods of the composition of the
complexes, as well as of the method used in the study of the
quantitative characteristics of the stepwise complex forma-
tion was extremely useful for all who attended this conference,
Card 16/16
USCM-DC-60976

V/
AUTHORS: Tvnanayev, IL. VY. , Petushkova, S. E. , 7-r-2130
ShpirTe_v_a,_6. 'V
TITLE: On the Preparation of Water-Free Lithium Iodide (0
poluchenii bezvodno6ro yodistogo lit-iya)
PERIODICAL: Zhurnal Neorganicheskoy Khimii, 1958, Vol 3 . Ur 5,
PP 1071-1074 (USSR)
ABSTRACT: Various methods for the preparation of lithium iodide
were tooted and are here described:
I..-Preparatiorl of lithiwa iodide by the application of
organic reaCents,
2. Immediate interaction between lithium and iodine,
3. Dehydration of lithium iodide in a HJ-current at 3000C,
4. Dehydration of lithium iodide melts in a vacuum.
All the above-m6ntioned methods gave unsatisfactory results.
In % apecial4r constructed vacuum destillation apparatus)
water-free lithium iodide was produced by heating its
watery salts in a vacuum at 600-850cC and at a pressure of
0,01 Hg. The water-free lithium iodide is highly hygro-
Card 1/2 scopic and decomposes under the influence of light.

On the Preparation of Water-Free Lithium Iodide 78-3-5-2/39
There are 1 figure and 5 references, 5 of which are Soviet.
SUBMITTED: May 21, 1957
AVAILABLE: Library of ConUre3s
1, LAM= iodide- FmIaraticn-Teat reaults
Card 2/2

,'47HORS: I. -.-VBokmellder, M. Ya. 78-3-6-1/30
TITLE: InvestiCations of the Reaction of the Production of Zircorium
Hydroxide (Issledovaniye reaktsii obrazovaniya gidrookisi
tsirkoniya)
PERIODICAL: Zhurnal Neorganicheskoy Khimii, 1958, Vol. 3, Nr 6,
pp. 1273 - 1260 (USSR )
ABSTRACT: In the present paper the process of formation of zirconium
hydroxide in the interaction between diluted solutions of
zirconium sulfate and zirconium oxichloride with soda lye is
investigated. The precipitation of zirconium hydroxide was
performed by means of the physico-chemical analyses, especially
by the methods of the solubility determination, the p H-deter-
minationg the determination of the electric conductivity and of
the volume of the zirconium hydroxide precipitations. It was
found in the investigations of the system Zr(so 4 )2_11a011-H20
that the reaction of zirconium sulfate with soda lye takes place
in three staCes. First, soluble, basic salt 3Zr(SO 4)2 Zr(OH)4
Card-1/2 forms, then the basic salt of the composition (ZrO.011)30 4

78-3-6-1/3o
InvestiCations of the Reaction of the Production of Zirconium Hydroxide
precipitates which at further addition of alkali hydroxide
passes into pure zirconium hydroxide.In the system
ZrOCI 2-NaOH-H 20 the formation of zirconiun hydroxide equally
takes place in three stages. First, soluble basic salt ZrO(OH)Cjl
forms, then the precipitation of the unstable basic salt
7ZrO(OH2 )ZrOO12precipitates which furthermore passe-s into the
hydroxide form under the action of NaOH. The zirconium hydr9xide
precipitations adsorb considerable quantities of alkalies from
the solution, which fact corresponds to the amphoteric character
of zirconium hydroxide. There are 12 figures, 2 tables Iand 21
references, 5 of which are 9oviet.
SUBMITTED- May 21, 1957
AVAILABLE: Library of CongTess
Card 2/2 1. Zirconium hydroxide--Production 2. Chemical reactions--Analysis

AUTHORS: Tananayev, 1. V., Leyifna, M. 1. SOV/78-"-9-8/78
TITLE: On Uranyl Ferrocyanides (0 ferrotsianidakh uranila)
PERIODICAL: Zhurnal neorganicheskoy khimii, 1956, Vol 3, Nr 9, pp 2045-2052
(USSR)
ABSTRACT: The interaction in an aqueous medium in the system UO 2(NO3)2 -
M4 [Fe(CN)6] - H 20 was investigated, wheiehl denotes Li ' Na, K, Rb
and ds. The investigations were carried out by determining the
solubilityi. by potentiometric determination, and by r -ecordin
the absorption spectrum. In the system UO (NO 3 )2 -Li 4[Fe(CN) 61
H 0 the normal uranyl ferrocyanide (U0 Fe(CN was eliminate
2 2) 2t], )6]
as solid phase. Also in the system UO 2(NO 3)2 -Na4[Fe(CN) 6] - H20
only normal uranyl ferrocyanide is formed. When adding a surpluf
of LiR and NaR colloidal solutions are formed. In the systems
with M Fe(CN) , where M denotes K, Rb, Cs, solid phases of th(
41 61
type M 4(U0 2) 4 [Fe (CN) 6j 3' as well as the solid intermediate phas,
Card 1/2 of the type M 2(UO2)3 LFe(r.N) 6J3 are formed. In the system with

On Uranyl Ferrocyanides
SOV/78-3-9-8/38
K [Fe(CN)~ in the presence of a surplus of the ion Fe(CN) 4-
4 11 6]
and K, ~-S% K SO the compound K Fe is formed.
2 4 12(U02)8 11 (CN)617
There are 4 figures, 4 tables, and 12 references, 7 of which
are Soviet.
SUBMITTED: November 29, 1957
Card 2/2

AUTHORS: -Jaaaa~~~~~vduyevskaya, K. A. SOV/78-3-9-26/36
TITLE: The Interaction in the System GeO 2-HF-H20 at a Temperature of
250C (0 vzaimodeystvii v sisteme GeO 2-HF-H20 pri 250)
PERIODICAL: Zhurnal neorganicheskoy khimii, 1958, Vol 3, Nr 9, pp 2165-2171
(USSR)
ABSTRACT: The forms and conditions of production of fluorine compounds
of germanium in the system GeO 2-HF-H20 were analyzed with
physico-chemical methods. The methods used were the determinatio
of solubility and electric conductivity. A diagram of solubility
in the system GeO 2-HF-H20 was established. In the case of an
HF con7tent of 0-35% there is a linearincrease of the solubilit3
of germr~nium oxide until a molar ratio of HF : GeO 2 - 4 is
reached. In the range of betwAn 35 and 41% HF the solubility
curve changes the direction: In this point a transformation of
GeF 4* 3H20 into,hexaflu-orine germanic acid - H2GeF 6* 2H20 -
takes place. By determining the solubility and electric con-
Card 1/2 duotivity, as well as the pH-value of the solution it was

SOV/78-3-9-26/38
The Interaction in the System GeO -HF-H 0 at a Temperature of 250C
2 2
shown that the compounds of the solid phase also exist in the
aqueous medium. In the system GeO 2-HF-H 20 only H2[GeOF4) and
H2[GeF6 are formed. Besides GeO2 also H 2 ~eOF 41-H20 and
H GeP .2H,O appear as solid phases in the system. The formatioi
2[ 61 C.
of these complex acids is confirmed by the determination of
electric conductivity. There are 5 figures, 6 tables, and 13
references, 3 of which are Soviet.
S'UBMITTED: July 24, 1957
Card 2/2

AUTHORS: Tananayev, I. V., Avduyevskaya, K. A. SOV/78-3-9-27/37e
TITLE: Analysis of the Interaction in the System GeO 2-H2C 204-H20
at 250C (Issledovaniye vzaimodeystviya v sisteme GeO 2-H 2C20 4-
H20 pri 250)
PERIODICAL: Zhurnal neorgan-4cheskoy khimii, 1958, Vol 3, Nr 9, pp 2172-2177
(USSR)
ABSTRACT: In the paper under review the interaction of GeO 2-H2C 204 in
aqueous solutions was analyzed by the potentiometric method as
well as by determining the electric conductivity and solubility
at 250C. In the interaction of germanium oxide and oxalic
acid the concentration of hydrogen ions increases. There is a
continuous increase of the concentration of hydrogen ions and
conductivity until. a ratio of H 20 204 : GeO 2 - 3 : 1 is reached,
after which it remains constant. The resulting conclusion is
that a complex of germanic acid with the formula H21Ge(C 204)31
exists in solution. The analyses of solubility at 250C sholned
that 0,045 mol per liter dissolve in o)calic acid. In a saturate
Card 1/3 solution of germanic acid with excess oxalic acid added

SOV/78-3-9-27/38
Analysis of the Interaction in the System GeO 2-rH 2C20 4-H20 at 250C
germanium oxalic acid crystallizes in colorless needle-shaped
crystals. This compound has the following composition:
H 2[Ge(C 204)3] .6H20. The result of the analysis was as follows:
Ge = 16,7%, C20 4 ~6oiq%, H 20 = 23,64%. In an acid medium
germanium oxalic acid exists as an ion only[Ge (C204 )3]2-. A
lessening of the acidity of the solution gives rise to ions
with a lower ratio of (C20 4)2- : Ge02* Thermograms of a complex
of germanium oxalic acid were recorded. At 430C an endothermic
effect occurs, which corresponds to the melting point of this
compound. Ammonium and potassium salts of germanium oxalic
acid were produced:(NH 4)2 [Ge(OH)2(C204)2]-3H20 and
K2[Ge(OH)2(C204)2j -3H20.
There are 5 figures, 3 tables, and 10 references, I of which -Is
Soviet.
SUBMITTED: April 7, 1958
Card 2/3

AUT11ORS: Tananayev, 1. V. , Ko,-Mi, Ya. L. 1-5-1-2 26
TITLE: The Investioation of the For.:,ation Reaction of Silver
Chloride and Silver Bromide by Means of th,-, Method of Liaht
Absorption (Issledovaniye reaktsiy obra:~ovaniya 1-.hlorida
i bromida serebra, metodom svetopogasheniya)
PERIODICAL: Zhurnal Analiticheskoy Khimii, 1958, Vol 13, 11r 1,
pP. 11-17 (USSR)
ABSTRACT: In an earlier paper (ref. 1) different systerzis with silver
iodide were investi-ated by measurin- li.-ht aboorption.
It was shovn that a connection exists between the solubility
of a suspension of J.gJ and its light absorption. In the
present article the results of the analogous investi,-.ations
of systems with silver bromide and silver chloride are
described. The composition of the precipitates in the systems
'10-110 - 'Llr - 11 0 and AIGNO-KC1 - 11 0 was investigated by
3 2 3 2
measurement of the light absorption. The clearly marked
maximum of the absorption of the developing suspension is
Card 1/5 attained at a concentration ratio A&110 3 : KX = 1(X - Br, Cl),

The Investi.-ation of the Formation Reaction of Silver Chloride 75-1-2/20"
and Silver Bromide by Yeanj of the Method of LiL;ht Absorption
The curve and with it also the degree of dispersion of the
precipitate is almost symmetrically modified toward both
sides of tho end point. Investigations of the systems
A~;Br - KBr - 1120 and A~- C1 - KC1 - 1120 showea that tin
increase in the concentration of the halogen ions causes an
increase in absorption which is explained by tht.! increase in
the solubility of the suspension by the addition of bromide
and chloride ions. In a comparison of the results obtained
with those already kno-i-,n for the xespective systems with
AGJ, the uniforra s"lape of the curves is remarkable. The
absorption maximuzi in all 3 systems is near similar values
of the concentration of the potassium halide, between 10 1
and 2.10-1 M-ol/liter. The absorption of a suspension of
AGC1 chan-,res only sli~;htly in concentrations of NaCl from
lo-3 tn 10-2 ';~ol/liter, whereas at hi~~hcr concentrations of
NaC1 the absorption increases rapidly. The rapid increase
in li~lit absorption takes place within the same concentratio::
ran-e of 7,TaCl where the solubility of silver chloride also
increases. When the quantity of the solid phn-ce
beco~ncs Llomewhat ICZL:, due to the incruasin. zolu'-ility, the
Card 2/5 valuo o-' '&1,c abzorption doess --ot The loss

'.',he Investigation of the Formation Reaction o-A" Silver Chloride 75-1-2/26
and Silver Bromide by Means of the Method of Liah-t Ab3ar2tion
of solid phase is compensated by an increase in absorption
based on an increase in particles. The investigation of the
systems AgBr - NH3 - U20 showed that after the addition of
very little ammonia to a suspension of silver bromide a
very rapid increase in light absorption takes place. A
comparison with the system AgJ - N113 - U20 showed great
differences which are due to the hiGhly different solubility
of AUJ and AgBr in NH8.
The system AgBr - Agif 3 - NH3 - H20 was investigated in
order to determine the influence of excess silver ions in
the presence of ammonia upon the absorption of a suspension
of silver bromide. It became evident that the nature of the
curves of light absorption as against the system without
excess AgNO~ does not change. In both cases the extinction
increases with increasing concentration of ammonia, runs
through a maximum, and then decreases to 0, corresponding to
a complete dissolution of AgBr. The higher the excess of
Ag'"3, the more does the domain of the maximum viden. There-
fore the complete dissolution of the precipitate is only
Card 3/5 attained at considerably higher concentrations of am-monia.
4 .

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1-4 eT Dl. Te 0-tv I t elle . aoll t-ric
a, Go%,P &Ijje of xg, -?~T 'a 1,.t e a3-1 e of
qjLj% 19 eo~ 0j&jV,
0-U TeB-t n M01:00'. eteli Tel OT teat ... Ge It -
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t1 ualto' el--Pe lb!-8-1-
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T eel Tw
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avas, gddd

The Investigation of the Formation Reaction of Silver Chloride 75-1-2/26
and Silver Bromide by '.'eans of the Method of Light Absorption
AVAILABLE: Library of Congress
1. 6ilver chloride - 'Ohemical reactions 2. 6ilver
bromide - Chemical reActions 3. Light -
Absorption - Neasurement
Card 5/5

AUTHORS: Deychman, E. N., Tananayev I. V. 75-13-2-7/27
TITLE: Determination of Small ~u-.antititea of Indium by Titriimp-
tric and Photometric 11uthodes (Opredeloniya malykh koli-
chestv indiya titri:~ietricheskini i fotoractriclieskim metow
dom')
PE'RIODICAL: Zhurnal 11naliticheskoy Kiiii-iii, 19513, Vol. 13, Nr 2,
pp. 196-2oo (USSR)
ABSTRACT: One of the best known titrimetric methods for the determi=
nation of indium. is based upon the potentiometric titration
by means of Potassium ferrocyanide (Refi 1). The composition
KIn5[Fe(CII)6] is ascribed to the compound formed here. Koll=
tgof (Ref. 2) says, however, that the composition of the
precipitating deposit was not yet investigated. In the in=
vestigation of the systems of indium chloride and of the
ferrocyanides of the alkalin6 metals (Refs. 3,4) it was
found that the following order applies for the tendency
to form mixed ferrocyanides with indium difficult to be
solved: Li~llla(K