If the ${K_{sp}}$ for $HgSO_4$ is $6.4 \times 10^{-5}$,then the solubility of the salt is:
- A$8 \times 10^{-3} \, M$
- B$8 \times 10^{-6} \, M$
- C$6.4 \times 10^{-5} \, M$
- D$6.4 \times 10^{-3} \, M$
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The solubility of $CaCl_2$ is $1.11 \times 10^{-8} \ g/100 \ mL$. If the molar mass of $CaCl_2$ is $111 \ g/mol$,find the $K_{sp}$.
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View SolutionThe correct order of solubility of the given salts in water at $298 K$ is:
Salt $K_{sp}$ at $298 K$ $AgBr$ $5.0 \times 10^{-13}$ $Zn(OH)_2$ $1.0 \times 10^{-15}$ $Hg_2Cl_2$ $1.3 \times 10^{-18}$
| Salt | $K_{sp}$ at $298 K$ |
| $AgBr$ | $5.0 \times 10^{-13}$ |
| $Zn(OH)_2$ | $1.0 \times 10^{-15}$ |
| $Hg_2Cl_2$ | $1.3 \times 10^{-18}$ |
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View SolutionWhich compound is soluble in $NH_4OH$?
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