The ${K_{sp}}$ of $Mg{\left( {OH} \right)_2}$ is $1.2 \times {10^{ - 11}}$ calculate its solubility in pure water.
$1.442 \times 10^{-4}$
The solubility product of $A{g_2}Cr{O_4}$ is $32 \times {10^{ – 12}}$. What is the concentration of $CrO_4^ – $ ions in that solution
In qualitative analysis, the metals of group $I$ can be separated from other ions by precipitating them as chloride salts. A solution initially contains $Ag^+$ and $Pb^{2+}$ at a concentration of $0.10 \,M.$ Aqueous $HCl$ is added to this solution until the $Cl^-$ concentration is $0.10\, M.$What will the concentrations of $Ag^+$ and $Pb^{2+}$ be at equilibrium ? ($K_{sp}$ for $AgCl = 1.8 \times 10^{-10},$$ K_{sp}$ for $PbCl_2 = 1.7 \times 10^{-5}$)
Which of the following does not give ppt with $CrO _{4}^{-2}$
Assertion : $KOH$ is more soluble in water than $NaOH$. Reason : $NaOH$ is a stronger base than $KOH.$
What is the molar solubility of $Al(OH)_3$ in $0.2\, M\, NaOH$ solution? Given that, solubility product of $Al(OH)_3 = 2.4 \times 10^{-24}$
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