Calculate the pH of a solution that contains 3.25 M HCN (K_a = 6.2*10^-¹⁰), 1.00 M NaOH and 1.50 M NaCN.

Name: Calculate the pH of a solution that contains 3.25 M HCN (K a = 6.2*10 - 10 ), 1.00 M NaOH and 1.50 M NaCN.
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Quizplus · Accepted Answer

The solution is a buffer containing HCN and its conjugate base CN-. Using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where pKa = -log(Ka) = 9.21. Substituting the concentrations, pH = 9.21 + log(1.50/3.25) = 9.25.

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