Autoionization of Water

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How can the concentration of hydroxide ions in a solution be expressed in terms of the pOH value?

$pOH = log[OH^-]$

$pOH = -log[OH^-]$ (correct)

$pOH = log[H^+]$

$pOH = -log[H^+]$

How does the net direction of an acid-base reaction depend on relative acid and base strengths?

The reaction proceeds to the lesser extent in the direction where a weaker acid and weaker base form a stronger acid and stronger base.

The reaction proceeds to the greater extent in the direction where a stronger acid and stronger base form a weaker acid and weaker base. (correct)

The reaction proceeds to the greater extent in the direction where a weaker acid and stronger base form a stronger acid and weaker base.

The reaction proceeds randomly without any relation to the strengths of the acids and bases involved.

What is one way to determine the strength of acids based on their pH values?

Acid strength increases as the pH value increases.

Acid strength remains constant regardless of the pH value.

Acid strength increases as the pH value decreases. (correct)

Acid strength is not related to the pH value of the solution.

What happens to the strength of an acid as its percent ionization increases?

The acid becomes stronger. Signup and view all the answers

What does percent ionization of an acid measure?

The proportion of ionized acid molecules in a solution compared to the initial concentration. Signup and view all the answers

How is the strength of a base determined from its pOH value?

$Base Strength = 14 - pOH$ Signup and view all the answers

What role does water play in reactions with acids?

It acts as both an acid and a base. Signup and view all the answers

What is the term for molecules or ions that can donate or accept a proton?

Amphiprotic species Signup and view all the answers

In the autoionization reaction of water, what do some water molecules do?

Act as acids by donating protons Signup and view all the answers

How does water behave when it reacts with the base NH3?

As an acid Signup and view all the answers

Which species is the most important amphiprotic species?

H2O Signup and view all the answers

What happens to a water molecule when it accepts a proton?

It becomes a base. Signup and view all the answers

What is the key variable that determines the concentration of H3O+ in the Henderson-Hasselbach equation?

Concentration of acid species Signup and view all the answers

In the Henderson-Hasselbach equation, what does pKa represent?

Concentration of conjugate acid Signup and view all the answers

What is the relationship described by the Henderson-Hasselbach equation for any conjugate acid-base pair?

Inverse proportionality between pH and pKa Signup and view all the answers

In a weak base dissociation, what does pKb represent?

Negative logarithm of base dissociation constant Signup and view all the answers

Which term in the Henderson-Hasselbach equation relates to the concentration of the weak acid?

[ weak acid ] Signup and view all the answers

What does the Henderson-Hasselbach equation enable the calculation of for a buffer solution?

pH of the buffer solution Signup and view all the answers

What is the pH of a buffer solution containing 0.1 M CH₃COOH and a 0.1 M solution of CH₃COONa?

4.5 Signup and view all the answers

If 1.0 mL of 0.10 M NaOH is added to 100 mL of the buffer in the first question, what will be the new pH?

10.0 Signup and view all the answers

When 1.0 mL of 0.10 M HCl is added to 100 mL of the buffer in the previous question, what is the resulting pH?

3.5 Signup and view all the answers

What is the purpose of a buffer solution?

To maintain a relatively constant pH when small amounts of acid or base are added Signup and view all the answers

Why is a buffer solution made using an acid-base conjugate pair?

To prevent the acid and base from neutralizing each other Signup and view all the answers

How can a simple buffer solution be prepared?

By adding comparable amounts of a weak acid and its conjugate base to water Signup and view all the answers

Why are the equilibrium concentrations of the acid and conjugate base assumed to be the same in a buffer solution?

Because the weak acid undergoes minimal hydrolysis Signup and view all the answers

What role do acetic acid and sodium acetate play in a simple buffer solution?

They help in maintaining the pH by acting as an acid-base conjugate pair Signup and view all the answers

Why should a buffer solution not consume the acid and base components in a neutralization reaction?

To prevent changes in pH Signup and view all the answers