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What is the effect of a larger KaK_a value?

Indicates a stronger acid and greater dissociation.

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What is the effect of a larger KaK_a value?

Indicates a stronger acid and greater dissociation.

What is the effect of a smaller KaK_a value?

Indicates a weaker acid and lesser dissociation.

What is the effect of a larger KbK_b value?

Indicates a stronger base and greater dissociation.

What is the effect of a smaller KbK_b value?

Indicates a weaker base and lesser dissociation.

What happens to the pH of a weak acid solution if the concentration of the weak acid is increased?

The pH will decrease because increasing the concentration of the weak acid will increase the [H⁺] in the solution.

Describe the general steps to solve for pH of a weak acid solution using an ICE table.

  1. Write the equilibrium reaction. 2. Set up the ICE table. 3. Write the KaK_a expression. 4. Solve for x (=[H⁺]). 5. Calculate pH = -log[H⁺].

Describe the general steps to solve for pH of a weak base solution using an ICE table.

  1. Write the equilibrium reaction. 2. Set up the ICE table. 3. Write the KbK_b expression. 4. Solve for x (=[OH⁻]). 5. Calculate pOH = -log[OH⁻]. 6. Calculate pH = 14 - pOH.

What is the Arrhenius definition of an acid?

Acids produce H⁺ ions in water.

What is the Arrhenius definition of a base?

Bases produce OH⁻ ions in water.

What is the Bronsted-Lowry definition of an acid?

Acids are proton (H⁺) donors.

What is the Bronsted-Lowry definition of a base?

Bases are proton acceptors.

Define a strong acid.

Acids that completely dissociate in water (virtually 100% ionization).

Define a strong base.

Bases that completely dissociate in water.

Define a weak acid.

Acids that incompletely dissociate in water; they exist in equilibrium between the undissociated and dissociated forms.

Define a weak base.

Bases that incompletely dissociate in water; they exist in equilibrium between the undissociated and dissociated forms.

Define chemical equilibrium.

A dynamic state where forward and reverse reactions occur at the same rate; there is no net change in concentrations of reactants and products.

What does a large equilibrium constant (K) indicate?

The reaction favors products.

What does a small equilibrium constant (K) indicate?

The reaction favors reactants.

Define KaK_a.

The acid dissociation constant; a measure of the strength of a weak acid. Ka=[H+][A−][HA]K_a = \frac{[H^+][A^-]}{[HA]}

Define KbK_b.

The base dissociation constant; a measure of the strength of a weak base. Kb=[BH+][OH−][B]K_b = \frac{[BH^+][OH^-]}{[B]}