Chemistry: Ka, Buffers & Equilibria Challenge

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Grade 11 Chem: Ka, buffers, and buffers effects

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Khouloud Abdelaziz

Saudi Arabia

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Froggy Jumps Chemistry: Ka, Buffers & Equilibria ChallengeOnline version Grade 11 Chem: Ka, buffers, and buffers effects by Khouloud Abdelaziz 1 1. What is the acid ionization constant (Ka)? a Equilibrium constant for the ionization of a weak acid b Total acid concentration in solution c Speed of acid-base reaction 2 2. In a 0.1 M weak acid solution, what percent ionizes roughly? a 98.7% b 50% c About 1.3% 3 3. Why is [H2O] omitted in the Ka expression? a Water does not participate in the reaction b Water is essentially constant as the solvent c Water is a solid here 4 4. For CH3COOH + H2O ⇌ H3O+ + CH3COO-, the Ka expression is: a Ka = [H3O+][CH3COO-] / [CH3COOH] b Ka = [H3O+][CH3COO-] / ([CH3COOH][H2O]) c Ka = [CH3COOH] / ([H3O+][CH3COO-]) 5 5. A weak acid is characterized by Ka being: a Relatively small b Very large c Exactly equal to 1 6 6. If initial weak acid concentration decreases, percent ionization generally: a Decreases b Increases c Remains constant 7 7. Temperature changes cause Ka to: a Always increase with temperature b Change to a new value at that temperature c Remain constant 8 8. Which measurement is most commonly used to determine Ka equilibrium concentrations? a Density b Mass c pH 9 9. In the derivation Ka = K[H2O], what does K represent? a The general equilibrium constant for the reaction b The pH of the solution c The acid ionization constant 10 10. In an acetic acid equilibrium, the three primary species present are: a CH3COO-, H3O+, Na+ b CH3COOH, H3O+, CH3COO- c CH3COOH, H2O, OH-

Froggy Jumps

Chemistry: Ka, Buffers & Equilibria ChallengeOnline version

Grade 11 Chem: Ka, buffers, and buffers effects

by Khouloud Abdelaziz

1. What is the acid ionization constant (Ka)?

Equilibrium constant for the ionization of a weak acid

Total acid concentration in solution

Speed of acid-base reaction

2. In a 0.1 M weak acid solution, what percent ionizes roughly?

98.7%

50%

About 1.3%

3. Why is [H2O] omitted in the Ka expression?

Water does not participate in the reaction

Water is essentially constant as the solvent

Water is a solid here

4. For CH3COOH + H2O ⇌ H3O+ + CH3COO-, the Ka expression is:

Ka = [H3O+][CH3COO-] / [CH3COOH]

Ka = [H3O+][CH3COO-] / ([CH3COOH][H2O])

Ka = [CH3COOH] / ([H3O+][CH3COO-])

5. A weak acid is characterized by Ka being:

Relatively small

Very large

Exactly equal to 1

6. If initial weak acid concentration decreases, percent ionization generally:

Decreases

Increases

Remains constant

7. Temperature changes cause Ka to:

Always increase with temperature

Change to a new value at that temperature

Remain constant

8. Which measurement is most commonly used to determine Ka equilibrium concentrations?

Density

Mass

9. In the derivation Ka = K[H2O], what does K represent?

The general equilibrium constant for the reaction

The pH of the solution

The acid ionization constant

10. In an acetic acid equilibrium, the three primary species present are:

CH3COO-, H3O+, Na+

CH3COOH, H3O+, CH3COO-

CH3COOH, H2O, OH-

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Chemistry: Ka, Buffers & Equilibria Challenge

Froggy Jumps

About this activity

Created by

Download the paper version to play

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Chemistry: Ka, Buffers & Equilibria ChallengeOnline version

by Khouloud Abdelaziz

1. What is the acid ionization constant (Ka)?

2. In a 0.1 M weak acid solution, what percent ionizes roughly?

3. Why is [H2O] omitted in the Ka expression?

4. For CH3COOH + H2O ⇌ H3O+ + CH3COO-, the Ka expression is:

5. A weak acid is characterized by Ka being:

6. If initial weak acid concentration decreases, percent ionization generally:

7. Temperature changes cause Ka to:

8. Which measurement is most commonly used to determine Ka equilibrium concentrations?

9. In the derivation Ka = K[H2O], what does K represent?

10. In an acetic acid equilibrium, the three primary species present are:

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