SUMMARY
The equilibrium constant for water, Kw, is 3.49e-13 at a specific temperature, indicating the concentration of hydrogen ions, [H+], in a neutral aqueous solution. By applying the equation Kw = [H+][OH-], it is determined that [H+] equals 3.49e-6. Consequently, the pH of the solution is calculated to be 5.457, confirming that Kw varies with temperature and affects the pH of neutral solutions.
PREREQUISITES
- Understanding of equilibrium constants in chemistry
- Knowledge of the relationship between pH and hydrogen ion concentration
- Familiarity with logarithmic functions
- Basic concepts of acid-base chemistry
NEXT STEPS
- Study the effects of temperature on Kw and pH
- Learn about the ion product of water at different temperatures
- Explore advanced acid-base equilibrium calculations
- Investigate the role of pH in chemical reactions
USEFUL FOR
Chemistry students, educators, and anyone interested in understanding acid-base equilibria and the impact of temperature on pH levels.