The $K_{sp}$ of $AgCl$ is $1.0 \times 10^{-10}$. Calculate the solubility of $AgCl$ in $0.2 \ M \ AgNO_3$.

The concentration of $500 \ mL$ $NaOH$ solution is $0.02 \ M$. How many grams of $FeSO_4$ must be added to this solution to initiate the precipitation of $Fe(OH)_2$? The $K_{sp}$ of $Fe(OH)_2$ is $1.5 \times 10^{-15}$. The molecular mass of $FeSO_4$ is $152 \ g \ mol^{-1}$.

Which of the following pairs of ions would be expected to form a precipitate when their solutions are mixed?

At $298 \ K$ temperature,the $K_{sp}$ of $CaF_2$ is $1.7 \times 10^{-10}$. If a person drinks $2.5 \ L$ of $CaF_2$ saturated water daily,how many grams of $CaF_2$ are present in the water consumed? (Molecular mass of $CaF_2$ is $78 \ g \ mol^{-1}$)

If $0.001435 \ g$ of $AgCl$ is present in $100 \ mL$ of water,calculate the $K_{sp}$.

The solubility product of $AgCl$ is $1.44 \times 10^{-4}$ at $100\,^{\circ}C$. The solubility of silver chloride in boiling water may be