A buffer solution of 100 mL contains both a weak acid HA and its sodium salt NaA, each at a concentration of 0.1 M. How many grams of solid NaOH must be dissolved in this buffer to raise the pH to 5.5? (Given: pKa of HA = 5; antilog(0.5) = 3.16)

Question

Accepted Answer

2.08 * 10⁻¹. Adding x mol NaOH converts HA to A⁻, shifting the [A⁻]/[HA] ratio. Setting pH = 5.5 in the Henderson-Hasselbalch equation and solving gives x = 0.005192 mol NaOH, which corresponds to 0.005192 * 40 = 0.2077 g ~ 2.08 * 10⁻¹ g.

A buffer solution of 100 mL contains both a weak acid HA and its sodium salt NaA, each at a concentration of 0.1 M. How many grams of solid NaOH must be dissolved in this buffer to raise the pH to 5.5? (Given: pKa of HA = 5; antilog(0.5) = 3.16)

Solution

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