The solubility product constants of $Ag_2CrO_4$ and $AgBr$ are $32x$ and $4y$ respectively at $298 \text{ K}$. The value of $(\frac{\text{molarity of } Ag_2CrO_4}{\text{molarity of } AgBr})$ can be expressed as :
- A$\frac{2\sqrt[3]{x}}{y}$
- B$2\sqrt{\frac{x}{y}}$
- C$\sqrt{\frac{x}{y}}$
- D$\frac{\sqrt[3]{x}}{\sqrt{y}}$
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Which of the following is the correct relationship between solubility $(S)$ and solubility product $(K_{sp})$ for silver oxalate?
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| Product | Sulphide Solubility $(K_{sp})$ |
|---|---|
| $I$ | $1.74 \times 10^{-16}$ |
| $II$ | $1.2 \times 10^{-22}$ |
| $III$ | $8.2 \times 10^{-46}$ |
| $IV$ | $5.0 \times 10^{-34}$ |
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