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its water content can be determined;<br />
<strong>the</strong> identification of <strong>the</strong> products<br />
that are produced by <strong>the</strong> reaction of<br />
NaK and components of <strong>the</strong> fuels; <strong>the</strong><br />
adaptation of a method for <strong>the</strong> de-<br />
termination of CeO in NaK; and <strong>the</strong><br />
adaptation of a method for <strong>the</strong> de-<br />
termination of UO, in UF,. A discus-<br />
sion of <strong>the</strong>se problems is included in<br />
<strong>the</strong> following paragraphs.<br />
zi reonium. An empirical volumetric<br />
method for <strong>the</strong> determination of zir-<br />
conium has been developed. The method<br />
is based on <strong>the</strong> measurement of <strong>the</strong><br />
basicity produced by <strong>the</strong> reaction<br />
between zirconium hydroxide and excess<br />
potassium fluoride, which was discussed<br />
in a previous report.(') Free acid in<br />
<strong>the</strong> starting solution in excess of<br />
0. 5 A' produced results approximately<br />
2% high. This interference can be<br />
overcome by dilution; a practical<br />
limit at ion must be imposed, however,<br />
because of <strong>the</strong> difficulty encountered<br />
in determining <strong>the</strong> end point. The use<br />
of acid media o<strong>the</strong>r than sulfuric acid<br />
was also explored. Only perchlorate<br />
systems were definitely unsatisfactory<br />
because of excessive hydrolysis at<br />
high ac idit y .<br />
Ano<strong>the</strong>r approach to <strong>the</strong> deve loprnent<br />
of a volumetric method for zirconium<br />
was to precipitate <strong>the</strong> hydroxide from<br />
a mineral acid solution with excess<br />
ammonium hydroxide, centrifuge, wash,<br />
and dissolve in standard acid; <strong>the</strong><br />
excess of standard acid was determined<br />
by titration. This method is satis-<br />
factory in an academic sense, but is<br />
hardly practical because of<strong>the</strong>copious<br />
washing required to free <strong>the</strong> hydrous<br />
oxide from basic salts and excess<br />
precipitant.<br />
The quantitative precipitation of<br />
zirconium by benzoic acid and nitro-<br />
benzoic acids has been reported.(2'3)<br />
(l)R. Rowan, Jr., J. C. White, C. M. Boyd,<br />
W. J. Ross, and C. K. Talbott, ANP Quar. Prog.<br />
Rep. Sept. 10. 1952, ORNL-1375, p. 159.<br />
("C, Lakshnan Rao, M. Venkataramaniah, and<br />
Bh. S. V. Raghava Rao, J. Sei. Ind. Research<br />
(India) IOR, NO. 7, 152-4 (1951).<br />
(3)M. Venkataramaniah and 5h. S. V. Raghava Rao,<br />
2. anal. Chen. 133, 248-51 (1951).<br />
PERIOD ENDING DECEMBER 10, 1952<br />
The reported method was used as a<br />
basis for formulating a volumetric<br />
method in which <strong>the</strong> precipltate is<br />
dissolved in dilute acid, and <strong>the</strong><br />
liberated organic acid is extracted<br />
with ethyl e<strong>the</strong>r and determined by<br />
titration in methyl alcohol-benzene<br />
solution with sodium methylate by<br />
using thymol blue as <strong>the</strong> indicator.<br />
However, a precipitate of varyink<br />
composition is formed, and attempts<br />
to establish an empl rical relationship<br />
were unsuccessful.<br />
Fur<strong>the</strong>r study of <strong>the</strong> reported<br />
gravimetric methods showed low results<br />
in all cases, <strong>the</strong> extent being de-<br />
pendent upon <strong>the</strong> nature of <strong>the</strong> medium<br />
of precipitation. For example, in a<br />
sulEate system, no precipitate 1s<br />
formed with benzoic acid because of<br />
<strong>the</strong> strength of <strong>the</strong> zirconium sulfate<br />
complex in solutions that are more<br />
acid than pH 3 to 4. A slight pre-<br />
cipitate was noted when m-nitrobenzoic<br />
acid was used as <strong>the</strong> precipitant.<br />
Nitric or hydrochloric acid solutions<br />
are recommended for this procedure.<br />
An attempt was made to titrate<br />
zirconium m-nitrobenzoate with per-<br />
chloric acid in ethylene glycol-<br />
isopropyl alcohol solution. Zirconium<br />
is not sufficiently basic in this<br />
medium, however, to give a distinct<br />
break in <strong>the</strong> potentiometric titration<br />
made by using a glass electrode as<br />
<strong>the</strong> indicator electrode and a calomel<br />
electrode as <strong>the</strong> reference electrode.<br />
Since mandelic acid gives a pre-<br />
cipitate of definite composition with<br />
zirconium, this reagent w i l l be<br />
studied for application to volumetric<br />
procedures.<br />
The effect of large excesses of<br />
uranium on <strong>the</strong> gravimetric determina-<br />
tion of zirconium was studied briefly<br />
in an attempt to select <strong>the</strong> precipitant<br />
least affected. Four reagents, phenyl-<br />
arsonic acid, mandelic acid, m-nitro-<br />
benzoic acid, and cinnamic acid, were<br />
tested on solutions of zirconium<br />
containing a fivefold excess of<br />
uranium. The number of determinations<br />
191