The table below shows the solubility (in M) of TICl in saturated TICl solution w

Question

The table below shows the solubility (in M) of TICl in saturated TICl solution with differing concnetrations of spectator ions, either from K2SO4 (left two columns) or KNO3 (right two columns).

[K2SO4] (M).............Solubility of TICl..................[KNO3] (M).......................Solubility of TICl

0..................................0.01607.................................0........................................0.01607

0.01.............................0.01779................................0.02...................................0.01716

0.025...........................0.01942................................0.05...................................0.01826

0.05..............................0.02137...............................0.1......................................0.01961

0.15..............................0.02600...............................0.3......................................0.02313

a) Explain why the solubility of TICl increases as the spectator ion concentration increases. this explanation will require the use of Debye-Huckel Theory.

b) Show that Debye Huckel Theory predicts that a plot of log(Solubiity) vs sqrt(I) should be a straight line.

c) Given that at Ksp is 1.86x10^-4, calculate activity coefficient gamma +/- as a function of ionic strength for the solutions with KNO3 (right two columns in table)

Explanation / Answer

The solubility of a salt in water can be influenced by the presence of other electrolytes in several ways: by a "common ion effect," by the occurrence of a chemical reaction involving one of the ions of the salt, or by a change in the activity

coefficients of the ions of the salt. The latter effect is caused by a change in the ionic strength of the solution, which

is related to the activity by the Debye-Huckel Theory.

The present experiment demonstrates the increase in solubility of Ca(IO3)2 in solutions containing KCl (a 1-1

electrolyte) of various concentrations. The increase in solubility is accounted for by Debye-Huckel Theory. An

equilibrium constant, Ks (in terms of activities), can be obtained by extrapolation of solubility data to zero concentration. The derived equilibrium constant can be used, in conjunction with experimental solubility data, to obtain

experimental values of ?

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