At 25^∘ C, the solubility of calcium oxalate, CaC2 O4, in water is 6.1 mg / L (a) What are the e

step 1 Calcium oxalate has a KSP value, so it has an equilibrium expression, where it dissociates into

At 25^∘ C, the solubility of calcium oxalate, CaC2 O4, in...

At $25^{\circ} \mathrm{C}$, the solubility of calcium oxalate, $\mathrm{CaC}_{2} \mathrm{O}_{4}$, in water is $6.1 \mathrm{mg} / \mathrm{L}$ (a) What are the equilibrium molar concentrations of $\mathrm{Ca}^{2+}(a q)$ and $\mathrm{C}_{2} \mathrm{O}_{4}{ }^{2-}(a q) ?$ (b) Calculate $K_{\mathrm{sp}}$ for calcium oxalate.

At $25^{\circ} \mathrm{C}$, the solubility of calcium oxalate, $\mathrm{CaC}_{2} \mathrm{O}_{4}$, in water is $6.1 \mathrm{mg} / \mathrm{L}$
(a) What are the equilibrium molar concentrations of $\mathrm{Ca}^{2+}(a q)$ and $\mathrm{C}_{2} \mathrm{O}_{4}{ }^{2-}(a q) ?$
(b) Calculate $K_{\mathrm{sp}}$ for calcium oxalate.

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Key Concepts

Conversion of Units in Solubility

When dealing with solubility expressed in units like mg/L, it is essential to convert these values into molar concentrations (mol/L) to relate to the equilibrium constant expressions. This conversion involves using the molar mass of the compound to convert the mass of the solute into the number of moles, which then allows for direct usage in calculating concentrations in the Ksp expression.

Dissolution Equilibrium

Dissolution equilibrium refers to the dynamic balance established when a sparingly soluble salt dissolves in water and simultaneously precipitates out of solution. At equilibrium, the rate of dissolution equals the rate of precipitation, and the concentrations of the ions produced are constant. The stoichiometric relationships in the balanced chemical equation dictate the ratio in which the ions appear in the solution.

Solubility Product Constant (Ksp)

The solubility product constant is an equilibrium constant that applies to the dissolution of sparingly soluble ionic compounds. It represents the product of the concentrations of the constituent ions, each raised to the power of their stoichiometric coefficients, when the solution is saturated. Ksp provides insight into the extent to which a compound dissolves in water, and a smaller Ksp indicates lower solubility.

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