The solubility product of Mg(OH)2 is 9.0 ×10^-12. The pH of an aqueous saturated solution of Mg(

step 1 Dear students, in the given multiple choice question, question number 99 of chapter 5, we have a

The solubility product of Mg(OH)2 is 9.0 ×10^-12. The pH of...

The solubility product of $\mathrm{Mg}(\mathrm{OH})_{2}$ is $9.0 \times 10^{-12}$. The $\mathrm{pH}$ of an aqueous saturated solution of $\mathrm{Mg}(\mathrm{OH})_{2}$ is $(\log 1.8=0.26, \log 3=0.48)$
(a) $3.58$
(b) $10.42$
(c) $3.88$
(d) $6.76$

Key Concepts

Logarithmic Relationships

Logarithms are used in chemistry to convert very small or large numbers into a more manageable form, most notably in the calculation of pH. The pH is defined as the negative logarithm of the hydrogen ion concentration, and similarly, pOH is defined for hydroxide ions, facilitating calculations with exponential values.

pH and pOH Relationship

The relationship between pH and pOH in aqueous solutions is given by the equation pH + pOH = 14 (at 25°C). This interdependence allows one to determine the pH of a solution by first calculating the hydroxide ion concentration and hence the pOH, then subtracting it from 14.

Solubility Product Constant (Ksp)

The Ksp quantifies the equilibrium between a sparingly soluble salt and its ions in solution. It is defined as the product of the molar concentrations of the dissociated ions, each raised to the power of their respective coefficients in the balanced dissolution equation. This value helps in calculating ion concentrations in a saturated solution.

Solubility Equilibrium

Solubility equilibrium refers to the state in which the rate of dissolution of a sparingly soluble salt equals the rate of its precipitation, resulting in a constant concentration of dissolved ions. This concept is critical for setting up the equilibrium expression that utilizes the Ksp to determine the extent of solubility of a compound.

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