A 50.00-mL solution of 0.0304 M ethanolamine (K_b = 3.2 $\times$10^-⁵)is titrated with a 0.0282 M solution of hydrochloric acid as the titrant.What is the pH of the base solution after 23.24 mL of titrant have been added? (K_w = 1.00 $\times$10^-¹⁴)

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After adding 23.24 mL of HCl, the solution is in the buffer region before the equivalence point. Use the Henderson-Hasselbalch equation to find the pH: pH = pKa + log([base]/[acid]). Calculate moles of ethanolamine and HCl, find concentrations, and use pKa = 14 - pKb to find pH.

A 5000-ML Solution of 0 ×\times× 10-5)is Titrated with a 0 ×\times×

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