SUMMARY
Ammonia (NH3) acts as a base in aqueous solution with a base dissociation constant (Kb) of 1.8 x 10-5. To find the acid dissociation constant (Ka) for the ammonium ion (NH4+), one must utilize the relationship Kw = Ka * Kb. Given that Kw (the ion product of water) is 1.0 x 10-14 at 25°C, Ka can be calculated by rearranging the equation to Ka = Kw / Kb.
PREREQUISITES
- Understanding of acid-base chemistry
- Familiarity with the concepts of Kb and Ka
- Knowledge of the ion product of water (Kw)
- Basic algebra for rearranging equations
NEXT STEPS
- Research the concept of Kw and its significance in acid-base equilibria
- Learn how to calculate Ka from Kb using the formula Ka = Kw / Kb
- Explore the properties of weak acids and bases in aqueous solutions
- Study the relationship between pH, pKa, and pKb in acid-base chemistry
USEFUL FOR
Chemistry students, educators, and anyone studying acid-base equilibria and the properties of ammonia and ammonium ions in aqueous solutions.