The ${K_{sp}}$ of $AgCl$ is $1.0 \times {10^{ - 10}}$ calculate solubility of $AgCl$ in $0.2$ $M$ $AgN{O_3}$.
$5 \times 10^{-10} \mathrm{M}$
Silver ions are added to a solution with $[Br^-] = [Cl^-] = [CO_3^{-2}]$ $= [AsO_4^{-3}] = 0.1\,M$. Which compound will precipitate with lowest $[Ag^+]$ ?
Solubility product of $BaC{l_2}$ is $4 \times {10^{ – 9}}$. Its solubility in moles/litre would be
What is the molar solubility of $Ag_2CO_3\, (K_{sp} = 4 \times 10^{-13})$ in $0.1\, M\, Na_2CO_3$ solution ?
If $K_{sp}$ of $CaF_2$ at $25\,^oC$ is $1 .7 \times 10^{-10},$ the combination amongst the following which gives a precipitate of $CaF_2$ is
The solubility product of silver sulphide is $3.2 \times {10^{ – 11}}.$ Its solubility at the experimental temperature is
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