3.46 mL x 2.37 M KOH = 8.20 mmoles.
26.9 mL x 1.78 M HCOOH = 47.88 mmoles.
............HCOOH + KOH ==> HCOOK + H2O
initial......8.20...47.88......0.......0
change.....-8.2....-8.2.....8.2.....8.20
final.......0.......40.68....8.20....8.20
You should recognize this as a buffered solution; i.e., it is a weak acid (HCOOH) with its salt (HCOOK). Use the Henderson-Hasselbalch equation to solve for pH.
What is the pH when 3.46 mL of 2.37 M KOH is added to 26.9 mL of a 1.78 M solution of formic acid (HCOOH)?
1 answer
1 answer