alleryIf the solubility of AgCl is s mol/L in pure water, then its Ksp is:
AThe simple value $s$ (only one factor)
B$s^2$ ($[Ag^+] \times [Cl^-]$ = $s \times s$)
C$2s^2$ (incorrect stoichiometry coeff)
DJust $s^3$ (wrong dissociation count)
Answer & Solution
Correct answer: B. $s^2$ ($[Ag^+] \times [Cl^-]$ = $s \times s$)
AgCl(s) ⇌ Ag+(aq) + Cl-(aq).
**At saturation:** [Ag+] = [Cl-] = s.
Ksp = [Ag+][Cl-] = s × s = s².
**So solubility s = √Ksp.**
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