A solution of nitrous acid (0.13 M, 20.00 mL) was titrated with 18.0 mL of 0.12 M sodium hydroxide (K_a of nitrous acid = 4.00 $\times$ 10^-4). What is the final pH of this solution?

Name: A solution of nitrous acid (0.13 M, 20.00 mL) was titrated with 18.0 mL of 0.12 M sodium hydroxide (K a of nitrous acid = 4.00 $\times$ 10 -4 ). What is the final pH of this solution?
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Question

Quizplus · Accepted Answer

The solution is a buffer after titration, and the pH can be calculated using the Henderson-Hasselbalch equation.

A Solution of Nitrous Acid (0 ×\times× 10-4)

A Solution of Nitrous Acid (0 $\times$ 10^-4)