SCIENTIFIC ABSTRACT GALKIN, N.P. - GALKIN, S.

• Document Type: CREST
• Collection: Scientific Abstracts
• Document Number (FOIA) /ESDN (CREST): CIA-RDP86-00513R000614120004-3
• Release Decision: RIF
• Original Classification: S
• Document Page Count: 100
• Document Creation Date: November 2, 2016
• Document Release Date: July 19, 2001
• Sequence Number: 4
• Publication Date: December 31, 1967
• Content Type: SCIENTIFIC ABSTRACT

27898
S/078/61/006/010/005/0 1
B121/B101
AUTHORS- Oalkin, N. P., Shubin, V. A., Krylov, it. S,
TITLE, "hemism of reduction of chemical uranium concentrates
-'L-RIODICAL: Zhurnal neorganicheakoy khimli, v. 6, no. 10, 1961, 2325-2328
TEXT: The authors deal with the problem of reducing uranium concentrates
obtained by ion exchange (85 % U 0 ) and containing Al and Fe impurities.
They studied the reduction of a;Mnium and sodium uranyl sulfates with
hydrogen in the presence of iron or aluminum oxides. The samples were
prepared by reacting NH 4OH or NaOH with UO 2so 4at a PH of 7-8 and a
temperature of 800C, and by adding the relevant Al or Fe cation. The
decomposition of ammonium urany' sulfate in a hydrogen atmosphere at
3500C obeys the equation: (NH4)2(UO2)2SO4 (OH)4 ), UO 2SO4+ UO3 +2NH 3 +3H20';
At 5500C, the UO 3 formed continues to decompose according to the equation:
5U03 ). U308 +1/2 02' U02 is formed front UO 31 U3 0., and uranyl sulfate by
reduction with hydrogen-, UO + H UO + H 0; U 0 + 2H - 5UO + ~H
3 2 2 2 3 8 2 2 4 2'1;
Card 1/3 A/

27898
S/078/6i/oo6/o1O/005/010
Chemism of reduction of chemical... B121/BIOI
U02 so 4 + 5"2 9 U02 + H2 S + 4H2 0. The decomposition of sodium uranyl sulfate
in a hydrogen atmosphere takes place according to the following equations:
Na 2(UO 2)2SO4 (OH) 4 '-, U 0 2so 4 + 2NaOH + UO 3 4 2H 2 0; 2NaOH +2UO Na2 U2 07 +H20;
UO2 so 4 +-2NaOH - Na 2so4 +UO 3 +R 20, The reduction of uranium (VI) from the
ammonium sal't takes place quantitatively, and uranium (VI) is reduced from
the sodium salt in an amount of 52.6 % only. Sodium diuranate was reduced
in order to study the effect of sodium on the reduction of uranium (VI)
compounds. Sodium diuranate is reduced in two stages:
Na2U2O 7 +H 2 ---.o-2NaUO 3 +H20; 2NaUO 3 + 112 2 UO 2 + 2NaOH.. Moreover,
reduction of the sulfates results in the formation of H 2 S which forms Na 2 S
with NaOR, The presence of sodium and iron interferes with the reduction
of uranium (VI). The reduction degree of uranium (VI) from ammonitim
uranyl sulfate in the presence of..irp a~t ~50oc is 64.6 %.after
;i hydroxidg
hr., The phase comoositi'o-n'of the reduction products in t'6'p'~'esence of
iron hydroxide was determined by x-ray analysis, UO 21 U 30.1 uranyl
sulfate-, and iron monouranate were found in the radiogram after a
Card 2/3

27895
S/078/61/006/010/005/010
Chemism of reduction of chemical-, B121./B101
r(Auoti.on time of 15 nin. 't 5530c, uranium (VI) of iron-containing
ammonium uranyl sulfatp is, almost entirely reduced by H2 after 4 hr UG 2?
FeS, and metallic Fe were the end products. The formation of iron sulfide
int-2rferes with the reduction of ammonium uranyl sulfate in the presence
of iron hydroxide. Aluminum hydroxide does not affect the reduction; it
behaves like a mechanical impurity. On reduction, the compounds studied
gave the same final compounds as are obtained by reduction of chemical
concentrates. There are 1 figure, 2 tables, and 3 references: 2 Soviet
and I non-Soviet. The reference to the English-language publication reads
as follows, Ch. D. Harringston, A. E. Ruehle. Uranium Production
Technology, New York, 1959,
SUBMITTED: SeDtember 14, 1960
Cara 3 3

"'93'
S/089/61/010/002/005/018
B102/B209
AUTHORS% GAlkin, N. P., Sudarikov, H. N. . Zaytaev, V. A., Vlasov, D. A.
TITLEs An investigation of the properties of uranium hexafluoride in
organic solvents
PERIODICAL: Atomnaya energiya, v. 10, no. 2, 1961, 143-148
TEXT: This is a report on investigations of the solubility and dissolution
kinetics of uranium hexafluoride in carbon tetrachloride, chloroform, di-
chloro-methane, unsymmetric dichloro-ethane, symmetric tetrachloro-ethane,
pentachloro-ethane, trifluoro-trichloro-ethane, symmetric trichloro-propane,
and tetrachloro-propane. The investigations of solubility were made in a
quartz container with a mixture of completely fluorinated hydrocarbons as
sealing liquidp at ~1400C. The kinetics of dissolution was determined at
250 in all organic solvents, except in dichloro-ethane, where it was made
at 10 0C. In the majority of the solvents, equilibrium was reached after
1 hour, in chloroform and trichloro-propane only after 3 hours. The values
Card 14

89355
s/oa9j'61/010/002/005/018
An investigation of the B102/B209
of UF6 solubility at 25 0G in the different solvents are listed in Table 1
(in g/ml).' Solubility increased monotonically with temperature, viz. lin-
early in the essential. The solubility of UP 4P U02F2 and 3N&F-UF6 in M 4
and CHC13 at 25 0C was also investigated and it was found to be!615 mg ura-
nium per liter; only 3NaF*UF 6 in M 4 had a solubility of 72 mg/l. The
solution Of UF6 in trifluoro-trichloro-ethane was colorless, whereas all
the other solutions were colored. In general, the color was intensified
with rising UP6 content. The stability of the solutions was determined at
200C. After a time of storage of 7 and 14 days in the exsiccator the ura-
nium content was determined; U IV was found in none of the cases. The re-
sults are compiled in Table 2. The stability in the case of a time of stor..
age of 30 days (200C) was examined, too. Table 3 shows the results. It
was found that the U IV content was practically independent of the solvent
and the initial UF6 concentration. Reduction of U VI proceeded faster in
chloroform and unsymmetrical C 2H4C1 2' After 7 days, 0.162 and 0.150 g U4+,
respectively, were found in 5 ml of solution (with 0.603 and 0.500 g UF 6
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8931515
8/089/61/010/002/005/018
An investigation of the B102/B209
initially). The degree of reduction was 27 ~& and/or 304,. Moreover, the
temperature dependence of the degree of reduction was ascertained. Table 6
shows data on the degree of reduction of UP6 (in j~). at 60, 90, and 10000 in
the individual solvents (3 ml solution, 048 9 UP6/ml), and Table.7 lists
the reduction degree and U VI/U IV ratio for several solvents. The inves-
tigations yielded the fdllowing results: 1) The chlorine derivatives of
methane are better solvents than the chlorine derivatives of ethane and
propane. 2) The solubility of UF6 and of uranyl fluoride in carbon tetra-
chloride and chloroform is very low. 3) At 200C, the solutions Of UF6 in
CC141 tetrachloro-ethane, pentachloro-ethane, and in trifluorq-triahloro-
ethane are stable, those in chloroform and dichloro-ethane are unstable.
4) In the reaction of UF6 with organic solvents, uranium pentaf-luoride forms,
which first is reduced to intermediate uranium fluorides and then to uranium
tetrafluoride. There are 4 figures, 7 tables, and 4 references! 3 Soviet-
bloc and 1 non-Soviet-bloo.
SUB14ITTED: April 14, 1960
Card 3/4

GALKIN, N.P.; SUDARIKOV, B.H.; ZAYTSEV, V.A.
Methods of reducing uranium hexafluoride. Atom. energ. 10 no.2:
149-155 P 161. (MIRA 14:1)
(Uranium fluoride)

i !A I Ili. -7 q I 1 11, 4 1;: 1
w1i Ht
&WW
s/08,,11/61/631 -0/00 ;1/00411021
1 08/E: 2 00
2
AUTHCRS. Galkin, K. P., Mayorov, A. A., Polonnikova, G. A.,
Sreherbakova, V. G., Utkina, L. V.
TITLE: Separation of uranium from impurities by means of
ammonium carbonate
PERIODICAL: Atomnaya energiya, v. 10, no. 3, 1961, 233-237
TEXT: The authors investigated the dissolution of pure (NH 4)2U207 in
(NH 4)2C03 and NH4HCO3, the separation of uranium in the form of
'he behavior of some imDurities in the salting out
(NH4) 41FUO 2(CO3)3j and4 -
of the crystals of this carbon complex. The dissolution involves the
following processes:
Card 1/,,K

Separation of uranium from
(NIi,)j'UjO, + 6(NH.,),,CO., + M20 4--*
2(NH,),,[UOI(COs)$'] + 6NHjOH;
(NH,),UO, + 6NH,HCOs 4-
2(NH.).[UO,(COs),j + 3H,O.
(1)
(2)
20174
S/08 61/010/0031/004/021
BlOBYB209
N,
The experiments were made with a special vessel in a thermostat at
40 + 0.10C. Equilibrium was practically reached after one hour. The
hi,g7her solubility of (NH 4)2U207 in NH4HCO3(Fig. 1) may be explained by
the action of NH 4OR which shifts the equilibrium to the left (see
reaction (1)). Dilute solutions containing (NH 4)2C03 or'NH4HCO 3 in a
stoichiometric ratio (according to (1) and (2)) may completely dissolve
ammonium di-uranate without formation of the.above carbon complex. The
precipitation of small and large crystals was determined in order to
study the influence of certain factors upon crystallization. Large
Card 24
I/

20174
S/089/61/010/003/004/021
Separation of uranium from ... B108/B209
crystals are called such of a size of 100 x20 - 300 Y-6o p. The experiments
were carried out as follows: (NE 4)2C03 was added under stirring to the
(NH4)41UO2(CO5)3] solution until saturation was reached. After salting
out had ceased, the solution with the crystals was stirred further on
for some time. The crystals were then filtered off and subjected to
sedimentation analysis. It was found that a temperature rise from
20 to 400C and an increase of the time of admixing (NH
lower the
CC)
)
2
4
3
quantity of small crystals. The same holds for an increase in the speed
of the stirrer from 60 to 160 rpm. However, a further increase has
hardly any effect. Fig. 7 shows the uranium concentration in the solution
during salting out of (NH 4)41UO2(CO3)31 - The best conditions of
crystallization are: temperature - 40 OC; time of (NH
admixture -
CO
)
2
3
4
1 hour; uranium concentration in the initial solution - 30 9/1; speed
of the stirrer - 180 rpm. The impurities to be investigated entered the
initial (ITH ) ruo (CO solution immediately before crystallization.
)
1
4 4L 2 3
3
The resulting ammonium di-uranate containing one kind of impurity was
Card 3/ 43
r

20174
S108 9/61/010/003/004/02 1
Separation of uranium from B108/B209
dissolved in a 5~.~ NH4HCO3solution. Under the above conditions, the
carbon complex crystallized. The filtered crystals were rinsed with a
saturated (NH 4)2CO3solution. After drying they were oxidized by anneal-
ing. Table 1 shows that most of the elements are easy to separate from
uranium. Table 2 shows the results of purification of ammonium di-uranate
which contained several kinds of impurities. There are 7 figures,
2 tables, and 3 references: 2 Soviet-bloc.
SUBMITTED: August 11, 1960
Card 4/jP
~4

S/089/61/010/003/018/021
B102/B205
AUTHORS: Galkin, N. P., Polonnikova, G. A.
I
TITLE: Separation of uranium from impurities by means of ammonium
sulfite
PERIODICAL: Atomnaya energiya, v. 10, no. 3, 19617 277-279
TEXT: Though the possibility of using (NH4)2SO, for uranium separation
has been known since 1843, there are no accurate methods available. The
authors believe that this substance is particularly suited for laboratory
work. The present "Letter to the Editor" deals with the conditions for
the purification of ammonium diuranate. The authors studied the
solubility of pure ammonium diuranate in ammonium-sulfite solution
dependent on various factors, as well as the cond. :rSation
4tions for the sep
of' uranium from an ammonium-sulfite solution. Specifically, they studied
the effect of the concentration of (NH 4)2 so 31 temperature, and the
T : a ratio (T - weight of wet diuranate; VtL-- weight of the ammonium-
sulfite solution) upon the solubility of ammonium diuranate in the
Card 1/4

Separation of uranium from impurities ... S/089/61/010/003/018/021
B102/B205
presence of (NH 4)2SO3' The dissolution took place according to the
reaction equation (NH 4)2U2 07 + 4(NH 4)2SO3 + 3H2 0,---P'2(NE 4)2 IU02 (SO 3)23
+ 61TH4OH. The experiments were carried out as follows: A weighed nor-
tion of pure ammonium diuranate of 56% moisture was introduced into
thick-walled test tubes, and a certain amount of freshly prepared
ammonium-sulfite solution was added. The tubes were stoppered and
mounted on a disk which was placed in an air thermostat. By perpendicular
rotation of the disk, the substance in the thermostat was intermixed.
The dissolution took 2 hr. The graphically reprearnted results show
that the solubility of ammonium diuranate increases wit *h an increase in
temperature and in the ratio of ammonium sulfite to uranium. The highest
uranium concentration in the solution reached in the experiments was
39.3 g/1 at an ammonium sulfite/uranium ratio of 14. A further expansion
of the volume of the (NH 4)2SO 3 solution led to a complete dissolution of
ammonium diuranate. The solubility of the diuranate can be increased by
neutralizing the forming ammonia with the help of sulfurous acid.
Card 2/4

SeDgration of uranium from impurities ... 5/089/61/010/003/018/021
B102/B205
Addition of 0-5 14 H SO per mole of uranium increases the uranium con-
2 3
tent in the solution from 16 to 28 g11, and addition of 1 M H so per
2 3
mole of uranium increases it to 52 g11 (T:'I'c- 1:2). Uranium can be
seDarated from ammonium-sulfiie solutions by boiling and keeping the
voiume of the solution constant. Deposits form at pH=6, one hour after
the solution has begun boiling. The deposits consist of coarse, yellow-
ish, transparent crystals. The ratio U : So : NH in the deposit was
3 3
determined to be I ; 1.96 : 2.'26. Optimum conditions for the dissolution
process: saturated ammonium-sulfite solution (concenturation of 320 g11),
temDerature of 800C, ammonium-sulfite to uranium ratio of 13.6, and
T:I.- = 1:2. The unsoluble deposit is fi'ltered off, and the solution is
boiled for 5 hr. The resulting crystals are washed twice in 10%
ammonium-sulfite solution, dried, and tempered at 800-9000C in order to
obtain a mixed uranium oxide. Results of an analysis of the initial aAd
3 tables,
the final product are contained in Table 3. There are 3 figurest
and 3 references: 1 Soviet-bloc and 1 non-Soviet-bloc.
SMITTED: August 4, 1960
Card-

Separation of uranium from impurities ... s/o89/61/010/003/018/021
B102/B205
Legend to Table 3:
1~ Product. 2) Content, % by weight. 3) Initial ammonium diuranate.
4 Mixed uranium oxide.
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