Determine the molar concentration of Cl^- ions in an equilibrium mixture containing 1.00 M PbCl₄^2- and 0.0010 M Pb^2- ions. Given: K_f = 2.5 $\times$ 10¹ for PbCl₄^2-.

Question

Quizplus · Accepted Answer

The correct answer is A because the molar concentration of ClF1F1F1S1^F1F1F10 ions in an equilibrium mixture containing 1.00 M PbCl₄²F1F1F1S1^F1F1F10 and 0.0010 M Pb²F1F1F1S1^F1F1F10 ions can be calculated using the equilibrium constant expression for the formation of PbCl₄²F1F1F1S1^F1F1F10 ions. The equilibrium constant expression is:K_f = [PbCl₄²F1F1F1S1^F1F1F10]/[Pb²F1F1F1S1^F1F1F10][Cl^-]⁴Substituting the given values into the equilibrium constant expression, we get:2.5 x 10¹ = [1.00]/[0.0010][Cl^-]⁴Solving for [Cl^-], we get:[Cl^-] = 0.628 MTherefore, the molar concentration of ClF1F1F1S1^F1F1F10 ions in the equilibrium mixture is 0.628 M.

Determine the Molar Concentration of Cl- Ions in an Equilibrium ×\times×

Determine the Molar Concentration of Cl^- Ions in an Equilibrium $\times$