What is the value for K_c for the following reaction: PbCl₂(s) ⇌ Pb²⁺(aq) + 2 Cl^-(aq) ,
If PbCl₂(s) = 1.50 grams,[Pb²⁺] = 1.6 × 10^-2 M and [Cl^-] = 3.2 × 10^-² M at equilibrium? (The molar mass of PbCl₂(s) is 278 g/mol and its density is 5.85 g/cm³. )

Question

Quizplus · Accepted Answer

The value for Ksp (solubility product constant) is calculated using the concentrations of the ions in solution at equilibrium. For the given reaction, Ksp = [Pb^2+][Cl^-]^2. Substituting the given concentrations, Ksp = (1.6 × 10^-2)(3.2 × 10^-2)^2 = 1.6 × 10^-5.

What Is the Value for Kc for the Following Reaction

What Is the Value for K_c for the Following Reaction