What is the minimum concentration of KOH required for precipitation to begin for each of the following cation solutions? a. 0.015 M CaCl2 b. 0.0025 M Fe(NO3)2 c. 0.0018 M MgBr2

Verified step by step guidance

Identify the relevant solubility product constant (K_sp) for each cation's hydroxide compound: Ca(OH)_2, Fe(OH)_2, and Mg(OH)_2.

Write the balanced chemical equation for the precipitation reaction of each cation with OH^- ions: Ca^{2+} + 2OH^- \rightarrow Ca(OH)_2, Fe^{2+} + 2OH^- \rightarrow Fe(OH)_2, Mg^{2+} + 2OH^- \rightarrow Mg(OH)_2.

Express the K_sp expression for each hydroxide: K_{sp} = [Ca^{2+}][OH^-]^2, K_{sp} = [Fe^{2+}][OH^-]^2, K_{sp} = [Mg^{2+}][OH^-]^2.

Substitute the given concentration of each cation into the K_sp expression to solve for the minimum [OH^-] required for precipitation: [OH^-] = \sqrt{\frac{K_{sp}}{[Ca^{2+}]}}, [OH^-] = \sqrt{\frac{K_{sp}}{[Fe^{2+}]}}, [OH^-] = \sqrt{\frac{K_{sp}}{[Mg^{2+}]}}, where [Ca^{2+}], [Fe^{2+}], and [Mg^{2+}] are the given concentrations.

Calculate the minimum concentration of KOH required, which is equal to the [OH^-] concentration found in the previous step, since KOH dissociates completely in solution.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of ionic compounds. It represents the maximum concentration of ions in a saturated solution at a given temperature. For precipitation to occur, the product of the ion concentrations must exceed the Ksp value of the compound being formed, indicating that the solution is supersaturated.

Precipitation Reaction

A precipitation reaction occurs when two soluble salts react in solution to form an insoluble compound, or precipitate. This process is driven by the formation of a solid that separates from the liquid phase. In the context of the question, KOH reacts with cations from the given solutions to form insoluble hydroxides, leading to precipitation.

Ion Concentration and Stoichiometry

Ion concentration refers to the amount of a specific ion present in a solution, typically expressed in molarity (M). Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. To determine the minimum concentration of KOH needed for precipitation, one must consider the stoichiometric ratios of KOH to the cations in the solutions and their respective solubility limits.

Recommended video:

Guided course

01:16

Stoichiometry Concept

Related Practice

Textbook Question

Predict whether a precipitate will form if you mix 75.0 mL of a NaOH solution with pOH = 2.58 with 125.0 mL of a 0.018 M MgCl₂ solution. Identify the precipitate, if any.

Textbook Question

Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. a. 0.035 M Ba(NO₃)₂; NaF

Textbook Question

Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. b. 0.085 M CaI₂; K₂SO₄

Textbook Question

Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. c. 0.0018 M AgNO₃; RbCl