Question

Predict if there will be any precipitate by mixing $50\,mL$ of $0.01\,M\, NaCl$ and $50\,mL$ of $0.01\,M\,AgNO_3$ solution. The solubility product of $AgCl$ is $1.5 \times 10^{-10}$.

• A. Since ionic product is greater than solubility product no precipitate will be formed
• B. Since ionic product is lesser than solubility product, precipitation will occur
• C. Since ionic product is greater than solubility product, precipitation will occur
• D. Since ionic product and solubility product are same, precipitation will not occur

Answer 1

Answer: (C)

$NaCl + AgNO_3 \rightarrow AgCl +NaNO_3$
$K_{sp}=1.5 \times 10^{-10}$
$\left[Ag^{+}\right]=\frac{1}{2}\times10^{-2}\,M=0.5\times10^{-2}\,M$
$\left[Cl^{-}\right]=\frac{1}{2}\times10^{-2}\,M=0.5\times10^{-2}\,M$
$K_{ip}=\left[Ag^{+}\right]\left[Cl^{-}\right]$
$=\left(0.5\times10^{-2}\right)\times\left(0.5\times10^{-2}\right)$
$=2.5\times10^{-5}$
$K_{ip} > K_{sp}$
When $K_{ip} > K_{sp}$, it results in precipitation.