SUMMARY
The discussion centers on calculating the pH at the equivalence point of a titration involving 0.0200 L of 0.100 M nitrous acid (HNO2) and 0.200 M sodium hydroxide (NaOH). The volume of NaOH required to reach the equivalence point is determined to be 0.01 L. At this point, the resulting solution will contain the conjugate base of nitrous acid, which will affect the pH. The pH can be calculated using the concentration of the conjugate base formed and its Kb value.
PREREQUISITES
- Understanding of acid-base titration concepts
- Knowledge of calculating equivalence points in titrations
- Familiarity with the properties of weak acids and their conjugate bases
- Ability to use the Kb value for nitrous acid to find pH
NEXT STEPS
- Calculate the pH of a solution using the Kb of nitrous acid
- Learn about the Henderson-Hasselbalch equation for buffer solutions
- Explore the differences between strong and weak acid-base titrations
- Study the concept of pH indicators and their application in titrations
USEFUL FOR
Chemistry students, educators, and laboratory technicians involved in acid-base titration experiments and pH calculations.