Molar Solubility from Ksp
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Finding molar solubility from Ksp means setting up an ICE table where dissolution produces x mol/L of each ion per its coefficient, substituting the equilibrium row into the Ksp expression, and solving algebraically for x, which equals the molar solubility of the solid itself once found and confirmed reasonable against the salt's generally known dissolution behavior in water.
For AgCl, Ksp = 1.8 × 10⁻¹⁰: [Ag+] = [Cl−] = x, so x² = 1.8 × 10⁻¹⁰, giving x ≈ 1.3 × 10⁻⁵ M as the molar solubility of the solid in pure water at this given fixed temperature.
For a salt like Ag2CrO4, the ion produced with coefficient 2 must be entered as 2x, not x, before squaring the full Ksp expression.