SUMMARY
The discussion focuses on calculating the specific conductivity (k) and resistance (R) of a solution containing 0.01 M hydrochloric acid (HCl) and 0.1 M acetic acid (HAc). The molar conductivity of HAc is given as Λm = 5.14 cm2S/mol, and the cell constant is Kcell = 0.5652. The relationship between conductivity and concentration is established through the equations k = c Λm and R = Kcell / k. The impact of adding a strong acid like HCl on the conductivity of HAc is also addressed, with the use of an ICE table being suggested as a method to simplify the calculations.
PREREQUISITES
- Understanding of molar conductivity and its calculation
- Familiarity with the concept of cell constants in conductivity measurements
- Knowledge of the ICE table method for equilibrium calculations
- Basic chemistry knowledge regarding strong and weak acids
NEXT STEPS
- Research the effects of strong acids on the conductivity of weak acids
- Learn how to construct and utilize ICE tables for equilibrium problems
- Study the relationship between concentration and conductivity in electrolyte solutions
- Explore the calculation of molar conductivity for different acids
USEFUL FOR
Chemistry students, educators, and professionals involved in analytical chemistry or solution chemistry who are looking to deepen their understanding of conductivity in mixed acid solutions.