6.11.3 - Ionization Constants of Weak Acids
Enroll to start learning
You’ve not yet enrolled in this course. Please enroll for free to listen to audio lessons, classroom podcasts and take practice test.
Practice Questions
Test your understanding with targeted questions
Define ionization constant (Ka).
💡 Hint: What does Ka measure?
What happens to the Ka of an acid when it is diluted?
💡 Hint: Think about the constants and their dependence on concentration.
4 more questions available
Interactive Quizzes
Quick quizzes to reinforce your learning
What does a larger Ka value indicate?
💡 Hint: Remember what Ka measures.
True or False: The ionization constant Ka changes with the concentration of the acid.
💡 Hint: Consider the nature of equilibrium constants.
Get performance evaluation
Challenge Problems
Push your limits with advanced challenges
A solution contains acetic acid and its sodium salt. How does this system illustrate the common ion effect? Discuss how pH changes when more acetate ion is added.
💡 Hint: Consider Le Chatelier's principle.
Calculate the Ka of a weak acid if its 0.1 M solution has a pH of 5.0.
💡 Hint: Convert pH to hydrogen ion concentration first.
Get performance evaluation
Reference links
Supplementary resources to enhance your learning experience.