At $298 \ K$,the solubility of silver chloride in water is $1.434 \times 10^{-3} \ g \ L^{-1}$. The value of $-\log K_{sp}$ for silver chloride is $........$ (Given: molar mass of $Ag = 107.9 \ g \ mol^{-1}$ and $Cl = 35.5 \ g \ mol^{-1}$)

Find the solubility in terms of $mol \ L^{-1}$ if the solubility product of silver bromide is $6.4 \times 10^{-13}$.

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

Calculate the solubility of $A_{2}X_{3}$ in pure water,assuming that neither kind of ion reacts with water. The solubility product of $A_{2}X_{3}$,$K_{sp} = 1.1 \times 10^{-23}$.

The solubility product of silver bromide $(AgBr)$ is $5.0 \times 10^{-13}$. What is the minimum amount of potassium bromide $(KBr)$ that must be added to $1 \ L$ of $0.05 \ M$ silver nitrate $(AgNO_3)$ solution to initiate the precipitation of $AgBr$? (Molar mass of $KBr = 120 \ g \ mol^{-1}$)

The solubility product of a sparingly soluble salt $AB$ at room temperature is $1.21 \times 10^{-6}$. Its molar solubility is