We’re being asked to calculate the pH of a buffer that is 0.020 M HF and 0.040 M NaF.
A solution that contains a weak acid and its conjugate base is a buffer solution. The pH of a buffer solution can be determined using the Henderson-Hasselbalch equation.
The solution is composed of 0.020 M HF and 0.040 M NaF.
• HF is a weak acid
• the anion in NaF is the conjugate base
Calculate the pH of a buffer that is 0.020 M HF and 0.040 M NaF? The Ka for HF is 3.5 × 10-4.
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