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

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

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

Write the equilibrium reaction. 2. Set up the ICE table. 3. Write the $K_a$ 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.

Write the equilibrium reaction. 2. Set up the ICE table. 3. Write the $K_b$ 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 $K_a$ .

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

Define $K_b$ .

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

What are the key differences between strong acids and weak acids?

Strong acids: Completely dissociate, have negligible conjugate base strength. | Weak acids: Partially dissociate, have conjugate bases with measurable strength.

What are the key differences between strong bases and weak bases?

Strong bases: Completely dissociate, have negligible conjugate acid strength. | Weak bases: Partially dissociate, have conjugate acids with measurable strength.

Compare and contrast $K_a$ and $K_b$ .

$K_a$ : Acid dissociation constant, measures acid strength. | $K_b$ : Base dissociation constant, measures base strength. | Both: Smaller values indicate weaker acids/bases.