Solid $Ba(NO_3)_2$ is gradually dissolved in $1\times10^{-4}\, M\, Na_2CO_3$ solution. At what concentration of $Ba^{+2}$ the precipitation of $BaCO_3$ will start? (If $K_{sp}$ of $BaCO_3 = 5.1\times10^{-9}$)

If ${K_{sp}}$ for $HgS{O_4}$ is $6.4 \times {10^{ – 5}},$ then solubility of the salt is

The solubility product of a binary weak electrolyte is $4 \times {10^{ – 10}}$ at $298\,K$. Its solubility in mol $d{m^{ – 3}}$ at the same temperature is

The required amount of $KBr$ (molar mass $= 119$ ) in gram to start the precipitation of $AgBr$ in $500\,mL$ solution of $0.05\,M\,\,AgNO_3$ will be :- ( $K_{SP}$ of $AgBr = 5 \times 10^{-13}$ )

Find the concentration of ion which is first precipitated at the point when the third ion starts precipitating, if $AgNO_3$ is added gradually to the solution that contains $0 .1\ M\  Cl^-, 0 .1\  M\ Br^-$ and $0. 1\ M\ I^-$

Given that

Salt            ||         $K_{sp}$

$AgCl$        ||        $2 \times {10^{ – 10}}$

$AgBr$       ||       $5 \times {10^{ – 13}}$

$Ag$           ||        $9 \times {10^{ – 17}}$