Question

5.0mL of 5.4 x 10⁻⁴ M cl- is added 5.0 mL of 3.8 x 10⁻⁷ M Agt. Total volume is now 10.0 mL, and each concentration has been been diluted diluted in half. Write the ion product expression (Qc) for Agcl and determine its value using the diluted Concentrations Compare Qc in part with KSP and determine what happens in that Agcl solution.

Answer 1

The ion product expression (Qc) for AgCl is calculated using the diluted concentrations of Ag+ and Cl-, revealing that Qc is less than the solubility product constant (Ksp). Hence, no precipitation of AgCl will occur in the solution.

Step-by-step explanation:

The question asks for the ion product expression (Qc) for AgCl and its value using the diluted concentrations of Ag+ and Cl- ions. It also asks to compare Qc with the solubility product constant (Ksp) to determine whether precipitation will occur.

Upon mixing the two solutions, each concentration is halved due to dilution, giving us [Cl-] = 2.7 x 10^-4 M/2 = 1.35 x 10^-4 M and [Ag+] = 1.9 x 10^-7 M/2 = 9.5 x 10^-8 M. The ion product Qc for AgCl is therefore Qc = [Ag+][Cl-] = (9.5 x 10^-8 M)(1.35 x 10^-4 M) = 1.2825 x 10^-11.

Comparing with the solubility product constant Ksp for AgCl, which is 1.6 x 10^-10, we find that Qc < Ksp. This means the solution is unsaturated with respect to AgCl and no precipitation will occur.