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(without typos) from the publisher. Not indexed. Not illustrated.
1897 Excerpt: ...other chloride in the same concentration. While it
is impossible to compute the theoretical value of the depression on
the basis of the dissociation theory, since measurements on the
conductivity of these solutions are wanting, it is, however, a
striking fact that if it be assumed that the salt at the
concentration m = 0.01 be completely dissociated, and that each
molecule splits up into the maximum number of five parts,
Sn-Cl-Cl-Cl-Cl, we would then have for the molecular depression
only 5 x 1.89 or 9.45, while the observed value is 12.61. Obviously
the depression is not to be explained in this way. It however
suggests itself that the SnCl4 does not exist at all in aqueous
solutions, but that it assumes at once the properties of a mixture
of SnCl2 and 2 HC1, in solution. No value for the depression of the
freezing-point by SnCl2 has been found; but assuming that it is
about that of CdCl2 and ZnCl2, as observed by Jones, i.e. 5.20, and
taking the observed value for HC1, i.e. 3.61, we have for the
depression due to SnCl4, 5.20+ 2(3.61), or 12.42. This is very
nearly the observed value. It should be said that many vain
attempts were made to prepare solutions of SnCl2, sufficiently free
from SnCl4, to enable the freezing-points to be measured. The
purpose was to measure the depressions in a solution of SnCl2 at m
= 0.01, and then add in succession a jfo grammolecule of HC1. Thus
measurements would be made on SnCl2, m = 0.01, SnCl2 + 1 HC1, in =
0.01, SnCl2 + 2 HC1, m = 0.01, SnCl2 + 3 HC1, m = 0.01, as was done
in the cases of the phosphates, p. 288. This would have decided
experimentally whether the suggestion just made in regard to the
nature of SnCl4 in solution is tenable. I hope to return to this
difficulty in the near future. It may be well to call atten...
|Country of origin:
American Institute of Physics
||246 x 189 x 8mm (L x W x T)
||Paperback - Trade
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