Calculate the pH of a buffer solution prepared by dissolving...

Calculate the $\mathrm{pH}$ of a buffer solution prepared by dissolving $21.46 \mathrm{~g}$ of benzoic acid $\left(\mathrm{HC}_{7} \mathrm{H}_{5} \mathrm{O}_{2}\right)$ and $37.68 \mathrm{~g}$ of sodium benzoate in $200.0 \mathrm{~mL}$ of solution.

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Key Concepts

Buffer Solution

A buffer solution is a system that resists changes in pH when small amounts of acid or base are added. It typically involves a weak acid and its conjugate base, which together can neutralize added ions to maintain a relatively constant pH.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a formula that relates the pH of a buffer solution to the pKa of the weak acid and the ratio of the concentrations of the conjugate base to the acid. It is a crucial tool for calculating the pH of buffer systems when the amounts of the acid and its salt are known.

Molarity and Stoichiometry

Molarity is the number of moles of a solute per liter of solution, and it is essential for preparing solutions and performing chemical calculations. Converting the mass of a compound to moles using its molar mass and then determining its concentration by dividing by the solution volume are key steps in working with buffer solutions.

Acid Dissociation Constant (pKa)

The pKa value indicates the strength of a weak acid, representing the pH at which the acid is half dissociated. It plays a critical role in buffer calculations as it is used in the Henderson-Hasselbalch equation to determine the pH based on the ratio of the conjugate base to the weak acid.

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