Which of the following formulas correctly represents the relationship between pH and the concentration of hydrogen ions?

A. pH = Log[H+]

B. pH = -Log[H+]

C. pH = [H+]

D. pH = 1/Log[H+]

If the pH of a solution is 5, how would you classify this solution?

A. Strongly acidic

B. Weakly acidic

C. Neutral

D. Basic

Which of the following is true about the relationship between pH and pOH?

A. pH + pOH = 14

B. pH - pOH = 7

C. pH * pOH = 14

D. pH / pOH = 2

What does a high pKa value for an acid indicate?

A. The acid is strong.

B. The acid is weak.

C. The acid is neutral.

D. The acid is basic.

Which of the following solutions has the lowest concentration of H+ ions?

A. pH 2

B. pH 5

C. pH 7

D. pH 9

a) Define the term pH and explain its significance in determining the acidity or basicity of a solution. [2]

b) A solution has a [H+] concentration of 1 x 10^-5 mol/L. Use the given formula to calculate its pH. [2]

a) Differentiate between strong and weak acids in terms of their pH values. [2]

b) If a strong acid has a pH of 2, what would be the [H+] concentration of the solution? [2]

a) Describe the relationship between pH and pOH in a solution. [2]

b) If a solution has a pOH of 8, determine its pH. [2]

a) Explain the significance of pKa in acid-base equilibria. [3]

b) A weak acid, HA, has a pKa of 4.5. If the pH of a solution containing this acid is 4.5, what can you infer about the concentrations of HA and A-? [2]

c) How would the pH of the solution change if more of the weak acid, HA, was added? [2]

a) Describe the difference between the degree of ionisation in strong and weak acids. [3]

b) Why do strong acids have a higher degree of ionisation than weak acids? [2]

c) If a strong acid is diluted, how does its degree of ionisation change? [2]

If the pOH of a solution is 3, what is its pH?

A. 3

B. 7

C. 11

D. 14

Which of the following is true about the significance of pKb for a base?

A. It indicates the strength of the base.

B. It indicates the concentration of the base.

C. It is the negative logarithm of the base's dissociation constant.

D. It is the positive logarithm of the base's dissociation constant.

A solution has a pOH of 4. What is the concentration of OH- ions in the solution?

A. 1 x 10^-4 M

B. 1 x 10^-10 M

C. 1 x 10^-7 M

D. 1 x 10^-14 M

Which of the following solutions is neutral?

A. pH 3

B. pH 5

C. pH 7

D. pH 9

If the pH of a solution decreases, what happens to the concentration of H+ ions?

A. It increases.

B. It decreases.

C. It remains the same.

D. It becomes zero.

a) What is the relationship between pOH and the concentration of hydroxide ions, [OH-]? [2]

b) Calculate the pOH of a solution if the concentration of [OH-] is 1 x 10^-3 mol/L. [2]

c) How does the pH of the solution relate to the pOH you calculated? [2]

a) Explain the concept of conjugate acid-base pairs. [3]

b) If NH3 acts as a base, what would be its conjugate acid? [2]

c) How does the strength of an acid relate to the strength of its conjugate base? [2]

a) Define pH and explain its significance in determining the acidic or basic nature of a solution. [3]

b) A solution has a pOH of 5. Calculate its pH. [2]

c) If the concentration of [H+] in a solution is 1 x 10^-4 mol/L, determine its pH. [2]

d) How would the addition of a strong base affect the pH of the solution? [2]

a) Describe the difference between pKa and pKb in the context of acid-base equilibria. [3]

b) A weak base, BOH, has a pKb of 3.2. If a solution of this base has a pOH of 3.2, what can be inferred about the concentrations of BOH and B+? [3]

c) How is the strength of a weak acid related to its pKa value? [2]

d) Given that the pKa of acetic acid is 4.76, calculate its Ka value. [2]

a) Explain the relationship between pH and pOH in a solution. [3]

b) A solution has a pH of 3. What is the concentration of H+ ions in the solution? [2]

c) If the concentration of OH- ions in a solution is 1 x 10^-10 mol/L, determine its pOH. [2]

d) How would the pH of the solution change if a strong acid is added? [2]