SUMMARY
The pH of a strong triprotic acid before titration can be determined by calculating the concentration of protons released upon complete dissociation. In this discussion, a 24 ml solution of 1.5 M unknown strong triprotic acid yields 0.036 moles of acid, resulting in 0.108 moles of protons. The concentration of protons is calculated using the formula [H+] = moles/volume, leading to a pH calculation that initially resulted in an incorrect value due to volume miscalculations. The correct approach emphasizes that strong acids dissociate completely, and the pH should be a positive value.
PREREQUISITES
- Understanding of strong acids and their complete dissociation in solution
- Knowledge of triprotic acids and their molecular structure (e.g., H3A)
- Familiarity with pH calculations and the formula pH = -log[H+]
- Basic skills in stoichiometry for calculating moles and concentrations
NEXT STEPS
- Research the properties and examples of strong triprotic acids
- Learn about pH calculations for polyprotic acids
- Study the concept of negative pH and its implications in chemistry
- Explore titration techniques and calculations for strong acid-base reactions
USEFUL FOR
Chemistry students, educators, and anyone interested in acid-base chemistry, particularly those studying titration and pH calculations of strong acids.