Upto what $pH$ must a solution containing a precipitate of $Cr{(OH)_3}$ be adjusted so that all of precipitate dissolves (When $C{r^{3 + }} = 0.1\,mol/\,l,\,{K_{sp}} = 6 \times {10^{ – 31}})$

Solid $Ba(NO_3)_2$ is gradually dissolved in a $1.0 \times 10^{-4}\, M$  $N_2CO_3$ solution. At what concentration of $Ba^{2+}$ will aprecipitate begin to form? ($K_{sp}$  for $BaCO_3 = 5 .1 \times 10^{-9}$)

$PbCl_2$ has max. concentration of $1.0\times10^{-3}\, M$ in its saturated aq. solution at $25\,^oC$. Its solubility in $0.1\, M\, NaCl$ solution will be

The ${K_{SP}}$ of $AgI$ is $1.5 \times {10^{ – 16}}$. On mixing equal volumes of the following solutions, precipitation will occur only with

In a saturated solution of the sparingly soluble strong electrolyte $AgIO_3$ (molecular mass $= 283$) the equilibrium which sets in is

$AgIO_{3(s)} \rightleftharpoons  Ag^+_{(aq)} +IO^-_{3(aq)}.$ 

If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1. 0 \times 10^{-8},$ what is the mass of $AgIO_3$ contained in $100\, ml$ of its saturated saolution ?