Question

Predict if there will be any precipitate by mixing $50mL$ of $0.01MNaCl$ and $50mL$ of $0.01MAgN{O}_3$ 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)

$NaCl+AgN{O}_3\to AgCl+NaN{O}_3$
$K_{sp}=1.5\times 10^{-10}$
$\left[A{g}^{+}\right]=\frac{1}{2}\times 10^{-2}M=0.5\times 10^{-2}M$
$\left[C{l}^{-}\right]=\frac{1}{2}\times 10^{-2}M=0.5\times 10^{-2}M$
$K_{ip}=\left[A{g}^{+}\right]\left[C{l}^{-}\right]$
$=\left(0.5\times 10^{-2}\right)\times \left(0.5\times 10^{-2}\right)$
$=2.5\times 10^{-5}$
$K_{ip}>K_{sp}$
When $K_{ip}>K_{sp}$, it results in precipitation.