SUMMARY
The pH of a solution prepared by mixing 50.0 mL of 0.300 M HCl with 450.0 mL of 0.400 M HIO3 is calculated to be 0.714. The calculation involves determining the new molarity of each acid after mixing, followed by applying the ICE (Initial, Change, Equilibrium) method to find the hydrogen ion concentration. The dissociation constant (Ka) for HIO3 is 1.6 x 10^-1, which influences the pH calculation. The final pH value is rounded to two significant digits due to the precision of the given Ka.
PREREQUISITES
- Understanding of acid-base chemistry, specifically strong and weak acids.
- Knowledge of the ICE method for equilibrium calculations.
- Familiarity with pH calculations and molarity concepts.
- Basic skills in performing dilution calculations.
NEXT STEPS
- Study the dissociation of strong vs. weak acids in aqueous solutions.
- Learn more about calculating pH for mixtures of strong and weak acids.
- Explore the implications of significant figures in chemical calculations.
- Investigate the use of the Henderson-Hasselbalch equation for buffer solutions.
USEFUL FOR
Chemistry students, educators, and professionals involved in analytical chemistry or laboratory work requiring pH calculations and acid-base equilibrium analysis.
