During a titration between a strong acid and a strong base, at what point is the pH equal to 7?

A. At the start of the titration

B. Halfway to the equivalence point

C. At the equivalence point

D. At the end of the titration

Which of the following combinations will result in a buffer solution during a titration?

A. Strong acid and its conjugate base

B. Weak acid and strong base

C. Strong acid and strong base

D. Weak acid and its conjugate base

In a titration between a weak acid and a strong base, where is the pH greater than 7?

A. At the start of the titration

B. Halfway to the equivalence point

C. At the equivalence point

D. At the end of the titration

Which of the following is NOT a characteristic of the buffer region in a pH curve?

A. It has a relatively flat portion of the curve

B. The pH changes slowly with the addition of titrant

C. It is where the equivalence point occurs

D. It can resist changes in pH

What is the pH at the equivalence point when titrating a weak base with a strong acid?

A. Less than 7

B. Equal to 7

C. Greater than 7

D. Cannot be determined

a) Explain the significance of the equivalence point on a pH curve during a titration. [2]

b) During the titration of a weak acid with a strong base, why does the pH at the equivalence point exceed 7? [2]

a) Describe the buffer region observed on a pH curve. [2]

b) Why is the pH change minimal in the buffer region even when a significant amount of titrant is added? [2]

a) How can the strength of an unknown acid be determined using a pH curve? [2]

b) Why is the initial pH lower in the titration of a strong acid with a strong base compared to the titration of a weak acid with a strong base? [2]

a) Define the terms Ka and Kb in the context of acid-base equilibria. [2]

b) How are Ka and Kb related to the ion product constant for water, Kw? [2]

c) If the Ka for an acid HA is 2.5 x 10^-5, calculate the Kb for its conjugate base A-. [3]

a) What is the significance of the half-equivalence point in a pH curve? [2]

b) How can one determine the pKa of a weak acid using its titration curve? [3]

c) Explain why the pH at the half-equivalence point is independent of the concentration of the weak acid. [2]

Which of the following combinations will have the steepest pH curve during titration?

A. Strong acid and weak base

B. Weak acid and weak base

C. Strong acid and strong base

D. Weak acid and strong base

In a titration, why is it important to identify the equivalence point?

A. To determine the concentration of the analyte

B. To know when the titration is complete

C. To calculate the pH of the solution

D. All of the above

Which indicator would be most suitable for a titration between a strong acid and a weak base?

A. An indicator that changes colour at pH 7

B. An indicator that changes colour at pH > 7

C. An indicator that changes colour at pH < 7

D. Any of the above

What is the main application of pH curves in titration analysis?

A. To visualise the change in pH during titration

B. To determine the end point of the titration

C. To identify buffer regions

D. All of the above

In a titration between a weak acid and a strong base, what happens to the pH when half of the acid has been neutralised?

A. The pH is equal to the pKa of the acid

B. The pH is equal to 7

C. The pH is half the pKa of the acid

D. The pH is twice the pKa of the acid

a) Describe the shape of a pH curve when a strong acid is titrated with a strong base. [3]

b) How does this shape differ when a weak acid is titrated with a strong base? [2]

c) Why is there a steep rise in pH near the equivalence point in both cases? [2]

a) What is the buffer region in a pH curve? [2]

b) Explain the role of a buffer solution in resisting changes in pH. [3]

c) How can one prepare a buffer solution using a weak acid and its salt? [2]

a) Describe the process of titration and its significance in determining the concentration of an unknown solution. [3]

b) Explain the term 'equivalence point' in the context of a titration curve. [2]

c) Given a weak base with a Kb of 3.2 x 10^-9, calculate its pKb. [2]

d) How can the pKb value help in determining the strength of a base? [3]

a) What is the significance of the endpoint in a titration? [2]

b) How does the endpoint differ from the equivalence point? [3]

c) Describe the role of an indicator in a titration experiment. [3]

d) Why is it crucial to choose an appropriate indicator for a specific titration? [2]

a) Explain the concept of a buffer region on a pH curve. [3]

b) How does a buffer solution maintain its pH upon the addition of a small amount of acid or base? [3]

c) Describe the difference in the pH curves when titrating a strong acid with a weak base versus a weak acid with a strong base. [3]

d) Why is the pH at the equivalence point not always 7 in acid-base titrations? [3]