The $K _{\text {s }}$ of $Ag _2 CrO _4$ is $1.1 \times 10^{-12}$ at $298 K$. The solubility (in $mol / L$ ) of $Ag _2 CrO$, in a $0.1 M AgNO _2$, solution is

The solubility product of $Mg(OH_2)$ is $1 \times 10^{-12}$. At what $pH$ precipitation will occur in $0.01\, M$ $MgCl_2$ solution?

A litre of solution is saturated with $AgCl$. To this solution if $1.0 \times {10^{ – 4}}$ mole of solid $NaCl$ is added, what will be the $[A{g^ + }]$, assuming no volume change

Solubility product of a sulphide $MS$  is $3 \times {10^{ – 25}}$ and that of another sulphide $NS $ is $4 \times {10^{ – 40}}$. In ammoniacal solution

Zirconium phosphate $[Zr_3(PO_4)_4]$ dissociates into three zirconium cations of charge $+4$ and four phosphate anions of charge $-3$. If molar solubility of zirconium phosphate is denoted by $S$ and its solubility product by $K_{sp}$ then which of the following relationship between $S$ and $K_{sp}$ is correct?