The solubility of Pb(OH)2 in water is 6.0 ×10^-6 M. The solubility of Pb(OH)2 in a buffer soluti

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The solubility of Pb(OH)2 in water is 6.0 ×10^-6 M. The...

The solubility of $\mathrm{Pb}(\mathrm{OH})_{2}$ in water is $6.0 \times 10^{-6} \mathrm{M}$. The solubility of $\mathrm{Pb}(\mathrm{OH})_{2}$ in a buffer solution of $\mathrm{pH}=8$ is (a) $8.64 \mathrm{M}$ (b) $2.16 \times 10^{-16} \mathrm{M}$ (c) $8.64 \times 10^{-16} \mathrm{M}$ (d) $8.64 \times 10^{-4} \mathrm{M}$

The solubility of $\mathrm{Pb}(\mathrm{OH})_{2}$ in water is $6.0 \times 10^{-6} \mathrm{M}$. The solubility of $\mathrm{Pb}(\mathrm{OH})_{2}$
in a buffer solution of $\mathrm{pH}=8$ is
(a) $8.64 \mathrm{M}$
(b) $2.16 \times 10^{-16} \mathrm{M}$
(c) $8.64 \times 10^{-16} \mathrm{M}$
(d) $8.64 \times 10^{-4} \mathrm{M}$

Key Concepts

Solubility Product Constant (Ksp)

The solubility product constant is a fixed value that represents the equilibrium between a sparingly soluble ionic compound and its constituent ions in solution. It is calculated by multiplying the ion concentrations (each raised to the power of its coefficient in the balanced dissolution equation) at equilibrium and is essential in predicting the solubility of a compound under various conditions.

Common Ion Effect

The common ion effect describes the decrease in solubility of a salt when a solution already contains one of the ions that the salt produces upon dissociation. This effect shifts the dissolution equilibrium towards the undissolved state, reducing the concentration of ions formed from the salt, and is a key concept in manipulating solubility equilibria.

Buffer Solutions and pH Control

Buffer solutions are designed to maintain a constant pH by resisting changes in hydrogen or hydroxide ion concentration when acids or bases are added. In the context of solubility, buffers can fix the concentration of a particular ion, such as OH–, which then influences the equilibrium position of a solubility reaction for a salt that produces that ion.

Equilibrium Calculations

Equilibrium calculations involve applying the law of mass action to a chemical system to determine the concentrations of all species at equilibrium. These calculations are essential for quantifying how factors like pH or the presence of common ions affect the solubility of compounds by manipulating the equilibrium conditions.

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