Use the given molar solubilities in pure water to calculate K_sp for each compound. a. BaCrO₄; molar solubility = 1.08⨉10^-5 M

Verified step by step guidance

1. Identify the dissolution equation for BaCrO_4: BaCrO_4(s) \rightleftharpoons Ba^{2+}(aq) + CrO_4^{2-}(aq).
2. Recognize that the molar solubility of BaCrO_4 is given as 1.08 \times 10^{-5} M, which means [Ba^{2+}] = 1.08 \times 10^{-5} M and [CrO_4^{2-}] = 1.08 \times 10^{-5} M at equilibrium.
3. Write the expression for the solubility product constant (K_{sp}): K_{sp} = [Ba^{2+}][CrO_4^{2-}].
4. Substitute the equilibrium concentrations into the K_{sp} expression: K_{sp} = (1.08 \times 10^{-5})(1.08 \times 10^{-5}).
5. Calculate the value of K_{sp} by multiplying the concentrations.

Key Concepts

Molar Solubility

Molar solubility is the maximum amount of a solute that can dissolve in a given volume of solvent at a specific temperature, expressed in moles per liter (M). It provides a quantitative measure of how much of a compound can be present in solution before reaching saturation. Understanding molar solubility is essential for calculating the solubility product constant (Ksp) of sparingly soluble salts.

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. It is defined as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced dissolution equation. Ksp provides insight into the extent to which a compound can dissolve in water and is crucial for predicting precipitation reactions.

Dissolution Equilibrium

Dissolution equilibrium refers to the dynamic balance between the solid phase of a solute and its ions in solution. For a compound like BaCrO4, the dissolution can be represented by a chemical equation where the solid dissociates into its constituent ions. At equilibrium, the rate of dissolution equals the rate of precipitation, allowing for the calculation of Ksp based on the concentrations of the ions in solution.