Which of the following formulas can be used to calculate the solubility of $Ag_2CO_3$?
- A$\sqrt{\frac{K_{sp}}{8}}$
- B$\sqrt[3]{\frac{K_{sp}}{4}}$
- C$\sqrt[3]{\frac{K_{sp}}{2}}$
- D$\sqrt[3]{\frac{K_{sp}}{8}}$
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View SolutionThe solubility of calcium carbonate $(CaCO_3)$ at $298 \ K$ is $6.4 \times 10^{-5} \ mol \ dm^{-3}$. Calculate the value of solubility product $(K_{sp})$ at the same temperature.
The solubility of sparingly soluble salt $AB_2$ is $1.0 \times 10^{-4} \ mol \ dm^{-3}$. What is its solubility product?
$A$ solution is saturated with $SrCO_3$ and $SrF_2$. The $[CO_3^{2-}]$ is found to be $1.2 \times 10^{-3} \ M$. The concentration of $F^{-}$ in the solution would be:
Given: $K_{sp}(SrCO_3) = 7.0 \times 10^{-10}$, $K_{sp}(SrF_2) = 7.9 \times 10^{-10}$
Given: $K_{sp}(SrCO_3) = 7.0 \times 10^{-10}$, $K_{sp}(SrF_2) = 7.9 \times 10^{-10}$
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View SolutionFor a compound $AB$,the degree of ionization is $80\%$. What is the solubility $(s)$ of $AB$ if its solubility product $(K_{sp})$ is $6.4 \times 10^{-9}$?
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