The solubility of PbCl2 when it is 80 % ionized is (a) 25 %...

The solubility of $\mathrm{PbCl}_{2}$ when it is $80 \%$ ionized is (a) $25 \%$ less than the solubility of $\mathrm{PbCl}_{2}$ when it is $100 \%$ ionized. (b) $50 \%$ less than the solubility of $\mathrm{PbCl}_{2}$ when it is $100 \%$ ionized. (c) More than the solubility of $\mathrm{PbCl}_{2}$ when it is $100 \%$ ionized. (d) is equal to the solubility of $\mathrm{PbCl}_{2}$ when it is $100 \%$ ionized.

The solubility of $\mathrm{PbCl}_{2}$ when it is $80 \%$ ionized is
(a) $25 \%$ less than the solubility of $\mathrm{PbCl}_{2}$ when it is $100 \%$ ionized.
(b) $50 \%$ less than the solubility of $\mathrm{PbCl}_{2}$ when it is $100 \%$ ionized.
(c) More than the solubility of $\mathrm{PbCl}_{2}$ when it is $100 \%$ ionized.
(d) is equal to the solubility of $\mathrm{PbCl}_{2}$ when it is $100 \%$ ionized.

Key Concepts

Solubility Product (Ksp)

The solubility product constant is an equilibrium constant used to describe the saturated solution of a sparingly soluble ionic compound. It is expressed as the product of the molar concentrations of the resultant ions, each raised to the power of their stoichiometric coefficients. Ksp is a fixed value at a given temperature and provides a key relationship between the solubility of the compound and the concentrations of its ions in solution.

Dissolution Equilibrium

Dissolution equilibrium refers to the dynamic balance that exists when a sparingly soluble salt dissolves in water and reaches equilibrium between the undissolved solid and the dissolved ions. In this state, the rate of the salt dissolving equals the rate of the ions recombining to form the solid. The dissolution equilibrium is governed by the solubility product constant, which links the total amount dissolved to the concentration of ions in solution.

Degree of Ionization

The degree of ionization describes the fraction or percentage of the dissolved compound that dissociates into its constituent ions in solution. For salts that do not completely ionize, the actual concentrations of free ions are reduced compared to the amount that would be present if 100% ionization occurred. This partial ionization affects the equilibrium concentrations and must be taken into account when calculating solubility using the Ksp expression.

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