What mass of $AgI$ will dissolve in $1.0 \ L$ of its saturated solution? [Given $: K_{sp}(AgI) = 1.0 \times 10^{-16} ; (At. \ wt. \ Ag = 108; I = 127)$]

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

Consider two Group $IV$ metal ions $X^{2+}$ and $Y^{2+}$. $A$ solution containing $0.01 \ M$ $X^{2+}$ and $0.01 \ M$ $Y^{2+}$ is saturated with $H_2S$. The pH at which the metal sulphide $YS$ will form as a precipitate is . . . . . . (Nearest integer). (Given: $K_{sp}(XS)=1 \times 10^{-22}$ at $25^{\circ} C$,$K_{sp}(YS)=4 \times 10^{-16}$ at $25^{\circ} C$,$[H_2S]=0.1 \ M$ in solution,$K_{a1} \times K_{a2}(H_2S)=1.0 \times 10^{-21}$,$\log 2=0.30, \log 3=0.48, \log 5=0.70$)

The $K_{sp}$ of $AgI$ is $1.5 \times 10^{-16}$. Precipitation will occur upon mixing equal volumes of which of the following solutions?

At $25 \, ^\circ C$,the $K_{sp}$ of $CaF_2$ is $1.7 \times 10^{-10}$. Which of the following combinations will result in the precipitation of $CaF_2$?

The solubility product constants $(K_{sp})$ of $CuS$,$Ag_2S$,and $HgS$ are $10^{-37}$,$10^{-44}$,and $10^{-54}$ respectively. The order of their solubility is: