Question

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

Since ionic product is greater than solubility product, precipitation will occur.

$NaCl\to N{a}^{+}+C{l}^{-}$

Number of mole of $C{l}^{-}=50ml\times 0.01=0.5$ milimol

$AgN{O}_3\to A{g}^{+}+N{O}_3^{-}$

Number of mole of $A{g}^{+}=50ml\times 0.01=0.5$ millimol

$\left[C{l}^{-}\right]=\frac{0.5}{50+50}=0.005M$

$\left[N{O}_3^{-}\right]=\frac{0.5}{50+50}=0.005M$

ionic product $=\left[A{g}^{+}\right]\left[C{l}^{-}\right]$

$=0.005\times 0.005$

$=2.5\times {10}^{-5}$

ionic product is greater than solubility product precipitation will occur