The solubility of AgCl in pure water at 25°C is $1.3 imes 10^{-5}$ M. Calculate its solubility (in M) in 0.1 M NaCl solution.

Two salts, $AB$ and $C_2D$, have the same $K_{sp}$ value of $1.0 imes 10^{-8}$ at 298 K. Which salt has the higher molar solubility?

For the precipitation of IInd group cations only the solution is made acidic so that:

Solubility of ${\rm{AgCl }}\;{\rm{at}}\;20^\circ C\;{\rm{ is}}\;1.435 imes {10^{ - 3}}\;g/L$. The solubility product of ${\rm{AgCl }}$ is

Solubility of ${\rm{AgCl }}\;{\rm{at}}\;20^\circ C\;{\rm{ is}}\;1.435 imes {10^{ - 3}}\;g/L$. The solubility product of ${\rm{AgCl }}$ is

The solubility of ${\rm{AgCl}}$ in 0.2 M${\rm\;{NaCl}}$ solution is$[{K_{sp}}\,of\,AgCl\,\,=\,\,1.2\,imes\,{10^{10}}]$

Some chemists at ISRO wished to prepare a saturated solution of a silver compound and they wanted it to have the highest concentration of silver ion possible. Which of the following compounds, would they use?

${K_{{\rm{sp}}}}\left( {{\rm{AgCl}}} \right) = 1.8 imes {10^{ - 10}}$

${K_{{\rm{sp}}}}\left( {{\rm{AgBr}}} \right) = 5.0 imes {10^{ - 13}}$

${K_{{\rm{sp}}}}\left( {{\rm{A}}{{\rm{g}}_2}{\rm{Cr}}{{\rm{O}}_4}} \right) = 2.4 imes {10^{ - 12}}$

Two sparingly soluble salts, AB and CD, have K$_{sp}$ values of 4 x 10$^{-10}$ and 1 x 10$^{-12}$ respectively. Which salt is more soluble?

When ammonium chloride is added to ammonia solution, the pH of the resulting solution will be

The solubility product of iron (III) hydroxide is $1.6 imes {10^{ - 39}}$. If $\;X$ is the solubility of iron (III) hydroxide, which one of the following expression can be used to calculate $\;X$?

${\rm{Zn}}$ salt is mixed with ${\left( {{\rm{N}}{{\rm{H}}_4}} \right)_2}{\rm{S}}$ of molarity $0.021\;M.$ The amount of ${\rm{Z}}{{\rm{n}}^{2 + }}$ remains unprecipitated in $12\;mL$ of this solution ${K_{sp}}\;of\;{\rm{ZnS}} = 4.51 imes {10^{ - 24}}$ which is: