The solubility of AgCl in 0.2 M NaCl soluti | vedclass

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(D) $AgCl(s) \rightleftharpoons Ag^+(aq) + Cl^-(aq)$ $NaCl(aq) \rightarrow Na^+(aq) + Cl^-(aq)$ Since $NaCl$ is a strong electrolyte,the concentration

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$6 	imes 10^{-10} \ M$

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(D) $AgCl(s) ightleftharpoons Ag^+(aq) + Cl^-(aq)$ $NaCl(aq) ightarrow Na^+(aq) + Cl^-(aq)$ Since $NaCl$ is a strong electrolyte,the concentration of $Cl^-$ ions from $NaCl$ is $0.2 \ M$. The solubility product expression is $K_{sp} = [Ag^+][Cl^-]$. Substituting the values: $1.20 	imes 10^{-10} = [Ag^+] 	imes 0.2$. Therefore,the solubility of $AgCl$ is $[Ag^+] = \frac{1.20 	imes 10^{-10}}{0.2} = 6 	imes 10^{-10} \ M$.

The solubility of $AgCl$ in $0.2 \ M \ NaCl$ solution ($K_{sp}$ for $AgCl = 1.20 \times 10^{-10}$) is:

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