QuestionEXAMPLE 7-5 Calculate the solubility of $\mathrm{Ba}\left(\mathrm{IO}_{3}\right)_{2}$ in a solution prepared by mixing 200 mL of $0.0100 \mathrm{M} \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}$ with 100 mL of 0.100 M NaIO .

Studdy Solution
Let $s$ be the solubility of $\mathrm{Ba}\left(\mathrm{IO}_{3}\right)_{2}$ in mol/L. At equilibrium: $$[\mathrm{Ba}^{2+}] = 0.00667 + s$$ $$[\mathrm{IO}_{3}^{-}] = 0.0333 + 2s$$
Assuming $s$ is small, approximate: $$[\mathrm{Ba}^{2+}] \approx 0.00667$$ $$[\mathrm{IO}_{3}^{-}] \approx 0.0333$$
Substitute into the $K_{sp}$ expression: $$K_{sp} = (0.00667)(0.0333)^2$$
Solve for $s$ using the known $K_{sp}$.
The calculated solubility $s$ will be the solubility of $\mathrm{Ba}\left(\mathrm{IO}_{3}\right)_{2}$ in the mixed solution.