Practice Ionization Constants Of Weak Acids (6.11.3) - Equilibrium

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6 sample questions

Question 1.
Define ionization constant (Ka).
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What does Ka measure?
Question 2.
What happens to the Ka of an acid when it is diluted?
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Think about the constants and their dependence on concentration.
3Question 3.
What does a larger Ka value indicate?
- A weaker acid
- A stronger acid
- No effect on acid strength
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Remember what Ka measures.
4Question 4.
True or False: The ionization constant Ka changes with the concentration of the acid.
- True
- False
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Consider the nature of equilibrium constants.
Question 5.
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.
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Consider Le Chatelier's principle.
Question 6.
Calculate the Ka of a weak acid if its 0.1 M solution has a pH of 5.0.
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Convert pH to hydrogen ion concentration first.

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