SUMMARY
The pH of a solution containing 0.1 M ammonia and 0.141 M ammonium chloride can be calculated using the Henderson-Hasselbalch equation. Given that the base dissociation constant (Kb) for ammonia is 1.8e-5, the solution acts as a buffer due to the presence of both the weak base (ammonia) and its conjugate acid (ammonium ions from ammonium chloride). The complete dissociation of ammonium chloride in water produces ammonium ions, which are essential for the buffer system.
PREREQUISITES
- Understanding of buffer solutions and their components
- Familiarity with the Henderson-Hasselbalch equation
- Knowledge of base dissociation constants (Kb)
- Basic concepts of acid-base chemistry
NEXT STEPS
- Study the Henderson-Hasselbalch equation in detail
- Learn how to calculate pH for buffer solutions
- Explore the properties and applications of ammonia as a weak base
- Investigate the dissociation of ammonium chloride in aqueous solutions
USEFUL FOR
Chemistry students, educators, and professionals involved in analytical chemistry or chemical engineering, particularly those focusing on buffer solutions and pH calculations.