Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na₂CrO₄ are added to 250 mL of 0.12 M AgNO₃? [K_sp(Ag₂CrO₄)= 1.1 × 10^-12] What is the concentration of the silver ion remaining in solution?

Question

Quizplus · Accepted Answer

The reaction between Na₂CrO₄ and AgNO₃ is:2Na₂CrO₄ + 2AgNO₃ → Ag₂CrO₄ + 4NaNO₃The K_sp for Ag₂CrO₄ is 1.1 × 10^-12. To determine if a precipitate will form, we can compare the ionic product (IP) of the solution to the K_sp. The IP is calculated by multiplying the concentrations of the ions in solution that are involved in the precipitation reaction. In this case, the ions are Ag⁺ and CrO₄^2-.[Ag⁺][CrO₄^2-] = (0.12 M)(0.33 M) = 3.96 × 10^-2 M²Since the IP (3.96 × 10^-2 M²) is greater than the K_sp (1.1 × 10^-12), a precipitate will form.To calculate the concentration of the silver ion remaining in solution, we can use the following equation:[Ag⁺] = K_sp/[CrO₄^2-][Ag⁺] = 1.1 × 10^-12/0.33 M = 2.9 × 10^-6 MTherefore, the correct answer is A: Yes, [Ag⁺] = 2.9 × 10^-6 M.

Which Response Has Both Answers Correct? Will a Precipitate Form