Will a precipitate form when 10.0 mL of 0.500 M NaCl is added to 10.0 mL of 0.0500 M AgNO₃? The K_sp for AgCl is 1.8 × 10^-10. A) Yes, because Q K_sp D) No, because Q K_sp

Question

Will a precipitate form when 10.0 mL of 0.500 M NaCl is added to 10.0 mL of 0.0500 M AgNO₃? The K_sp for AgCl is 1.8 × 10^-10. A) Yes, because Q < K_sp B) Yes, because Q = K_sp C) Yes, because Q > K_sp D) No, because Q < K_sp E) No, because Q > K_sp

Quizplus · Accepted Answer

When mixing the solutions, the concentration of Ag+ and Cl- ions in the final solution must be calculated to determine the reaction quotient (Q) and compare it with the solubility product constant (Ksp) for AgCl. The final volume of the mixture is 20.0 mL, and the final concentrations of Ag+ and Cl- are 0.025 M and 0.250 M, respectively. The reaction quotient Q = [Ag+][Cl-] = (0.025 M)(0.250 M) = 6.25 × 10^-3, which is greater than the Ksp of AgCl (1.8 × 10^-10). Therefore, a precipitate of AgCl will form because the product of the ion concentrations exceeds the solubility product, indicating that the solution is supersaturated with respect to AgCl.

Will a Precipitate Form When 10