Question

Calculate the concentration of each ion remaining in solution after precipitation is complete. Assume that the precipitate is completely insoluble. Concentration of K⁺= ___M Concentration of OH⁻ = ___M Concentration of Mg²⁺ = ____M Concentration of NO₃⁻ = ____M

A 764.0 mL aliquot of 0.440 M aqueous potassium hydroxide is mixed with 764.0 mL of 0.440 M aqueous magnesium nitrate. Write a balanced chemical equation for any reaction that occurs.

Answer 1

The question involves calculating ion concentrations after a precipitation reaction and comparing the ion product with the solubility product constant (Ksp) to determine if precipitation will occur.

Step-by-step explanation:

The student's question is about calculating concentrations of ions after precipitation is complete in a chemistry context, and the chemical reaction equation that occurs when two solutions are mixed together. The equation for the reaction when aqueous potassium hydroxide is mixed with aqueous magnesium nitrate is:

2KOH(aq) + Mg(NO3)2(aq) → Mg(OH)2(s) + 2KNO3(aq)

The procedure involves combining the initial concentrations and volumes of K+, OH−, Mg2+, and NO3− ions and calculating the final concentrations after the precipitation of Mg(OH)2.

For the ion product and Ksp comparison, the question involves different concentrations and substances like Mg2+ and F− but uses a similar approach:

Ion product = [Mg2+][F−]2

This product is compared with the Ksp value to determine if the precipitation occurs.