The molar solubility of Zn(OH)2 in 1 M ammonia solution at room temperature is (Ksp. of Zn(OH)2=

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The molar solubility of Zn(OH)2 in 1 M ammonia solution at...

The molar solubility of $\mathrm{Zn}(\mathrm{OH})_{2}$ in $1 \mathrm{M}$ ammonia solution at room temperature is $\left(K_{\mathrm{sp}}\right.$ of $\mathrm{Zn}(\mathrm{OH})_{2}=1.6 \times 10^{-17} ; K_{\text {stab }}$ of $\left.\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}^{2+}=1.6 \times 10^{10}\right)$ (a) $4 \times 10^{-3} \mathrm{M}$ (b) $1.58 \times 10^{-6} \mathrm{M}$ (c) $4 \times 10^{-9} \mathrm{M}$ (d) $2.56 \times 10^{-7} \mathrm{M}$

The molar solubility of $\mathrm{Zn}(\mathrm{OH})_{2}$ in $1 \mathrm{M}$ ammonia solution at room temperature is $\left(K_{\mathrm{sp}}\right.$ of $\mathrm{Zn}(\mathrm{OH})_{2}=1.6 \times 10^{-17} ; K_{\text {stab }}$ of
$\left.\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}^{2+}=1.6 \times 10^{10}\right)$
(a) $4 \times 10^{-3} \mathrm{M}$
(b) $1.58 \times 10^{-6} \mathrm{M}$
(c) $4 \times 10^{-9} \mathrm{M}$
(d) $2.56 \times 10^{-7} \mathrm{M}$

Key Concepts

Solubility Product Constant (Ksp)

The solubility product constant, or Ksp, is a numerical value that expresses the equilibrium between a sparingly soluble solid and its constituent ions in a saturated solution. It is defined as the product of the concentrations of the ions each raised to the power of its stoichiometric coefficient in the dissolution reaction. Understanding Ksp is essential in predicting whether a precipitate will form and in calculating the solubility of a compound under equilibrium conditions.

Stability Constant (Formation Constant)

The stability constant, often denoted as Kstab or Kf, quantifies the strength of a complex ion formed in solution. It represents the equilibrium constant for the reaction where a metal ion combines with ligands to form a complex. A high stability constant suggests that the complex is very stable, meaning that the metal ion is largely sequestered by the ligands. This concept is crucial when predicting how complex formation can enhance the solubility of an otherwise poorly soluble compound.

Coupled Equilibria in Solubility

Coupled equilibria occur when two or more equilibrium processes are interconnected within the same system. In solubility problems, the dissolution equilibrium of a sparingly soluble salt can be coupled with an additional equilibrium involving complex ion formation. The formation of a complex ion can shift the equilibrium of the dissolution process, typically enhancing solubility by removing one of the products from the initial dissolution equilibrium. Understanding these interactions is key to solving problems where multiple equilibria dictate the overall solubility of a compound.

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