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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 \(K_a\) 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.
1. 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 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.
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. \(K_b = \frac{[BH^+][OH^-]}{[B]}\)