Ksp = [Ag⁺][Cl⁻]
1.8 × 10⁻¹⁰ = [Ag⁺][0.1]
[Ag⁺] = 1.8 × 10⁻⁹ M
Ksp = [Pb²⁺][Cl⁻]²
1.7 × 10⁻⁵ = [Pb²⁺][0.1]²
[Pb²⁺] = 1.7 × 10⁻³ M

Question

Accepted Answer

Both values. The solubility product expressions for AgCl and PbCl₂ are correctly solved, yielding [Ag⁺] = 1.8 × 10⁻⁹ M and [Pb²⁺] = 1.7 × 10⁻³ M. Thus, both values are correct.

Ksp = [Ag⁺][Cl⁻] 1.8 × 10⁻¹⁰ = [Ag⁺][0.1] [Ag⁺] = 1.8 × 10⁻⁹ M Ksp = [Pb²⁺][Cl⁻]² 1.7 × 10⁻⁵ = [Pb²⁺][0.1]² [Pb²⁺] = 1.7 × 10⁻³ M

Solution

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