SUMMARY
The calculation of pH for a 0.15 M solution of potassium hydroxide (KOH) involves using the ionization of strong bases and the ion product of water (Kw). The hydroxide ion concentration is determined as [OH-] = 0.15 M, leading to a pOH of 0.824. The pH is then calculated using the relationship pH + pOH = 14, resulting in a final pH of 13.18. This method confirms the strong base's complete ionization in dilute solutions.
PREREQUISITES
- Understanding of strong base ionization
- Knowledge of pH and pOH calculations
- Familiarity with the ion product of water (Kw)
- Basic logarithmic functions
NEXT STEPS
- Study the properties of strong bases and their ionization in solution
- Learn about the ion product of water (Kw) and its significance in acid-base chemistry
- Explore advanced pH calculation techniques for various concentrations
- Investigate the effects of temperature on Kw and pH calculations
USEFUL FOR
Chemistry students, educators, and anyone involved in laboratory work or research related to acid-base chemistry and pH calculations.