SUMMARY
The pH at halfway to the equivalence point in the titration of 25.00 mL of 0.20 mol/L formic acid (HCO2H) with 0.26 mol/L sodium hydroxide (NaOH) can be calculated using the Henderson-Hasselbalch equation. At this point, 0.0025 moles of formic acid remain, and the concentration of its conjugate base, formate (HCO2-), is equal to that of the acid. The pH is determined to be equal to the pKa of formic acid, which is approximately 3.75.
PREREQUISITES
- Understanding of titration concepts and equivalence points
- Familiarity with the Henderson-Hasselbalch equation
- Knowledge of acid-base chemistry, specifically weak acids and their conjugate bases
- Basic skills in stoichiometry for calculating moles and concentrations
NEXT STEPS
- Study the Henderson-Hasselbalch equation in detail
- Learn about the properties and applications of weak acids and their conjugate bases
- Explore titration curves and how to interpret them
- Investigate the pKa values of common weak acids
USEFUL FOR
Chemistry students, educators, and laboratory technicians involved in acid-base titrations and pH calculations.