Calculate the pH of a 0.050 M Al(NO3)3 solution. The Ka...

Calculate the $\mathrm{pH}$ of a $0.050 \mathrm{M} \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}$ solution. The $K_{\mathrm{a}}$ value for $\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}$ is $1.4 \times 10^{-5}$.

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Key Concepts

pH Calculation

The pH of a solution is determined by the concentration of hydrogen ions present and is calculated as the negative logarithm of the [H+]. This concept connects the equilibrium analysis of acid dissociation directly to the measurable acidity of a solution.

Weak Acid Equilibrium Calculations

This involves setting up the equilibrium expression for the dissociation of a weak acid, applying approximations (like assuming a small degree of dissociation), and solving for the concentration of hydrogen ions. These calculations are essential for determining the pH of solutions containing weak acids.

Complex Ion Hydrolysis

This concept involves the reaction of a metal ion coordinated with water molecules undergoing a reaction with water (hydrolysis) to release protons, thereby making the solution acidic. It is fundamental in understanding why certain salts, especially those containing highly charged metal ions, result in acidic solutions.

Acid Dissociation Constant (Ka)

The acid dissociation constant quantifies the extent to which a weak acid, such as a metal-aquo complex, donates its proton to form its conjugate base. It is a critical parameter in determining the degree of hydrolysis and the resulting production of H+ ions in solution.

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