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Answer :
The pH of the buffer solution prepared by adding 5.00 g of sodium acetate and 5.00 g of acetic acid to water with a total volume of 50.0 mL is approximately 4.76.
To determine the pH of the buffer solution, we need to consider the dissociation of acetic acid and the reaction between acetic acid and sodium acetate.
Acetic acid (CH₃COOH) is a weak acid that partially dissociates in water, releasing hydrogen ions (H+). Sodium acetate (CH₃COONa) is the salt formed from the reaction between acetic acid and sodium hydroxide. It dissociates completely in water, releasing acetate ions (CH₃COO-) and sodium ions (Na+).
The acetate ions can react with the hydrogen ions from the partial dissociation of acetic acid, forming undissociated acetic acid and water. This reaction helps maintain the pH of the solution.
The buffer solution acts as a reservoir of both acetic acid and acetate ions, allowing it to resist large changes in pH when small amounts of acid or base are added.
By calculating the concentrations of acetic acid and acetate ions in the buffer solution, we can determine the pH using the Henderson-Hasselbalch equation: pH = pKa + log([CH₃COO-]/[CH₃COOH]).
Given the initial amounts of sodium acetate and acetic acid, the buffer solution's pH is approximately 4.76.
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