The two salts BaCl2 and Ag2SO4 are both far more soluble in water than either BaSO4 (Ksp= 1.1 × 10-10) or AgCl (Ksp= 1.6 × 10-10) at 25°C. Suppose 50.0 mL of 0.040 M BaCl2(aq) is added to 50.0 mL of 0.020 M Ag2SO4(aq). Calculate the concentrations of SO42- (aq), Cl2(aq), Ba2+(aq), and Ag+(aq) that remain in solution at equilibrium.

The two salts BaCl2 and Ag2SO4 are both far more soluble in water than either BaSO4 (Ksp= 1.1 × 10-10) or AgCl (Ksp= 1.6 × 10-10) at 25°C. Suppose 50.0 mL of 0.040 M BaCl2(aq) is added to 50.0 mL of 0.020 M Ag2SO4(aq). Calculate the concentrations of SO42- (aq), Cl2(aq), Ba2+(aq), and Ag+(aq) that remain in solution at equilibrium.

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Chapter16: Acid-base Equilibria

Section: Chapter Questions

Problem 16.154QP

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