If the solubility product of AgCl is 10^{-10} | vedclass

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(D) The dissociation of $AgCl$ is: $AgCl(s) ⇌ Ag^+(aq) + Cl^-(aq)$.Let the solubility of $AgCl$ be $s \ mol/L$.$NaCl$ is a strong electrolyte and diss

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$10^{-7}$

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(D) The dissociation of $AgCl$ is: $AgCl(s) ⇌ Ag^+(aq) + Cl^-(aq)$.Let the solubility of $AgCl$ be $s \ mol/L$.$NaCl$ is a strong electrolyte and dissociates completely: $NaCl(aq) → Na^+(aq) + Cl^-(aq)$.Concentration of $Cl^-$ from $NaCl$ is $0.001 \ M$.Total concentration of $[Cl^-] = (s + 0.001) \ M \approx 0.001 \ M$ (since $s$ is very small).$K_{sp} = [Ag^+][Cl^-] = s 	imes 0.001 = 10^{-10}$.$s = \frac{10^{-10}}{10^{-3}} = 10^{-7} \ M$.

If the solubility product of $AgCl$ is $10^{-10}$,what is the solubility of $AgCl$ in $0.001 \ M \ NaCl$?

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