Write a balanced chemical equation for the equilibrium...

Write a balanced chemical equation for the equilibrium occurring when each of these solutes is added to water, then write the $K_{\mathrm{sp}}$ expression for each solute. (a) $\mathrm{BaCrO}_{4}$ (b) $\mathrm{Mn}(\mathrm{OH})_{2}$ (c) Lead(II) carbonate (d) Nickel(II) hydroxide (e) Strontium phosphate (f) Mercury(I) sulfate

Write a balanced chemical equation for the equilibrium occurring when each of these solutes is added to water, then write the $K_{\mathrm{sp}}$ expression for each solute.
(a) $\mathrm{BaCrO}_{4}$
(b) $\mathrm{Mn}(\mathrm{OH})_{2}$
(c) Lead(II) carbonate
(d) Nickel(II) hydroxide
(e) Strontium phosphate
(f) Mercury(I) sulfate

Key Concepts

Dissolution Equilibrium

Dissolution equilibrium refers to the reversible process in which a sparingly soluble salt dissolves in water to produce its constituent ions. At equilibrium, the rates of the dissolution and precipitation processes are equal, which allows the solubility level of the salt to be described by its solubility product constant (Ksp).

Balanced Chemical Equations

Writing balanced chemical equations is essential when representing chemical equilibria as it ensures conservation of mass and charge. Each ionic species in the equilibrium must be correctly quantified, as the stoichiometric coefficients directly affect the mathematical form of the equilibrium constant expression.

Solubility Product Constant (Ksp)

The solubility product constant, Ksp, is an equilibrium constant specific to sparingly soluble salts. It is defined as the product of the molar concentrations of the constituent ions, each raised to a power equal to its coefficient in the balanced dissolution equation. This constant helps predict the extent of dissolution and the formation of precipitates under various conditions.

Stoichiometry in Equilibrium Expressions

Accurate stoichiometry in the dissociation reaction is crucial because the balanced equation not only shows the proportion of ions formed but also determines the exponents used in the Ksp expression. This relationship is fundamental to predicting solubility and understanding the effects of changes in concentration on the equilibrium.

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