Answer :

Final Answer:

The pH of the buffer solution prepared by adding 2.00 g of NH₄Cl(s) and 2.00 g of NH₄OH(l) is approximately 9.25.

Explanation:

A buffer solution is a solution that can resist changes in pH when an acid or base is added to it. In this case, the buffer is formed by the ammonium ion (NH₄⁺) from NH₄Cl and the ammonia molecule (NH₃) produced when NH₄OH dissociates.

The initial concentrations of NH₄⁺ and NH₃ can be calculated using the given masses and molar masses of the substances. Next, using the Henderson-Hasselbalch equation:

[tex]\[ \text{pH} = \text{pKa} + \log\left(\frac{\text{[NH₃]}}{\text{[NH₄⁺]}}\right) \][/tex]

The pKa for the ammonium ion (NH₄⁺) is approximately 9.25. Substituting the concentrations into the equation, we find the pH of the buffer solution. The log term dominates the equation due to the similar concentrations of NH₃ and NH₄⁺ in a well-designed buffer, leading to a pH close to the pKa.

In this scenario, the pH of the buffer solution is approximately 9.25, indicating that the solution is basic. This is consistent with the nature of ammonium buffers, which resist changes in pH against the addition of acidic substances and tend to maintain a slightly basic environment.

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Rewritten by : Barada