SUMMARY
The % ionisation of hypochlorous acid (HClO) in a 0.015M solution at 25°C is calculated to be 0.14%. The acid dissociation constant (Ka) for HClO is 3.0 x 10^-8. The calculation involves setting up an equilibrium expression using the formula \(\frac{{[x][x]}}{{0.015 - x}} = Ka\), where x is the concentration of ionized HClO. The discussion highlights the use of ICE tables for solving equilibrium problems.
PREREQUISITES
- Understanding of acid dissociation constants (Ka)
- Familiarity with equilibrium expressions in chemistry
- Knowledge of ICE (Initial, Change, Equilibrium) tables
- Basic logarithmic calculations for pH and ionisation
NEXT STEPS
- Study the application of ICE tables in equilibrium calculations
- Learn how to derive and use the Henderson-Hasselbalch equation
- Explore the concept of weak acid ionisation and its implications in buffer solutions
- Investigate the effects of concentration changes on the % ionisation of weak acids
USEFUL FOR
Chemistry students, educators, and anyone studying acid-base equilibria, particularly those focusing on weak acids and their ionisation properties.