Question

Determine the pH at the equivalence point in the titration of 41.0 mL 0.096 M formic acid with 0.108 M NaOH at 25oC.

Calculate the pH of a solution that is 0.22 M pyridinium ion (C5H5NH+) at 25oC.
What is it that you don't understand about the problem? The pH at the equivalence point of formic acid and NaOH is determined by the hydrolysis of the salt, i.e., sodium formate.

Related Questions

It says prepare a theoretical titration of 25 mL of 0.1037 M formic acid (HCOOH; pKa= 3.75) solution... Prepare a theoretical titration curve for titration of 25.0 mL of 0.1037 formic acid (HCOOH; pKa = 3... Consider the titration of 20.00 mL of 0.1728 M Ascorbic acid (Ka = 7.9 x 10-5) with 0.4329 M NaOH.... When 50 mL of 0.10M formic acid, HCHO2, is titrated with 0.10M sodium hydroxide, what is the pH at t...