Q1 / 150 · MHT CET 2026 (17 April Shift 2) · Chemistry
Which of the following is correct relationship between solubility and solubility product for silver oxalate ?
- A$S = \sqrt[3]{K_{sp} \times 4}$
- B$S = \sqrt[3]{\dfrac{4}{K_{sp}}}$
- Correct answerC$S = \sqrt[3]{\dfrac{K_{sp}}{4}}$
- D$S = \sqrt[4]{\dfrac{K_{sp}}{27}}$
Solution
The chemical formula of silver oxalate is $Ag_2C_2O_4$.
The dissociation reaction is:
$Ag_2C_2O_4(s) \rightleftharpoons 2Ag^+(aq) + C_2O_4^{2-}(aq)$
Let the solubility of silver oxalate be $S$.
Then, $[Ag^+] = 2S$ and $[C_2O_4^{2-}] = S$.
The solubility product $K_{sp}$ is given by:
$K_{sp} = [Ag^+]^2 [C_2O_4^{2-}]$
Substituting the concentrations:
$K_{sp} = (2S)^2 (S) = 4S^3$
$S^3 = \dfrac{K_{sp}}{4}$
$S = \sqrt[3]{\dfrac{K_{sp}}{4}}$
Answer: $S = \sqrt[3]{\dfrac{K_{sp}}{4}}$
The dissociation reaction is:
$Ag_2C_2O_4(s) \rightleftharpoons 2Ag^+(aq) + C_2O_4^{2-}(aq)$
Let the solubility of silver oxalate be $S$.
Then, $[Ag^+] = 2S$ and $[C_2O_4^{2-}] = S$.
The solubility product $K_{sp}$ is given by:
$K_{sp} = [Ag^+]^2 [C_2O_4^{2-}]$
Substituting the concentrations:
$K_{sp} = (2S)^2 (S) = 4S^3$
$S^3 = \dfrac{K_{sp}}{4}$
$S = \sqrt[3]{\dfrac{K_{sp}}{4}}$
Answer: $S = \sqrt[3]{\dfrac{K_{sp}}{4}}$
Hence, the correct answer is option: 'C'.