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 effect of a larger $K_a$ value?

Indicates a stronger acid and greater dissociation.

What is the effect of a smaller $K_a$ value?

Indicates a weaker acid and lesser dissociation.

What is the effect of a larger $K_b$ value?

Indicates a stronger base and greater dissociation.

What is the effect of a smaller $K_b$ 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.

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.

All Flashcards

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 effect of a larger $K_a$ value?

Indicates a stronger acid and greater dissociation.

What is the effect of a smaller $K_a$ value?

Indicates a weaker acid and lesser dissociation.

What is the effect of a larger $K_b$ value?

Indicates a stronger base and greater dissociation.

What is the effect of a smaller $K_b$ 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.

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.