question_answer 26)

Calculate the solubility of \[{{A}_{2}}{{X}_{3}}\] in pure Water, assuming that neither kind of ion reacts with water. The solubility product of\[{{A}_{2}}{{X}_{3}},{{K}_{sp}}=1.1\times {{10}^{-23}}\].

Answer:

\[{{A}_{2}}{{X}_{3}}\to 2A_{2s}^{3+}+3X_{3s}^{2-}\] \[{{K}_{sp}}={{[{{A}^{3+}}]}^{2}}{{[{{X}^{2-}}]}^{3}}\] \[={{(2s)}^{2}}{{(3s)}^{3}}=108{{s}^{5}}\] \[s={{\left( \frac{1.1\times {{10}^{-23}}}{108} \right)}^{1/5}}\] (Solve using log table.) \[=1\times {{10}^{-5}}mol/litre\]