Chemistry Quiz: Acid-Base Buffer Solutions

What is the everyday English definition of a buffer?

• A solution that lessens the change in [H3O+] when a strong acid or base is added

• A concentrated solution of a strong acid and base

• A substance that increases the impact of an external force

• A substance that has no effect on external forces

Tags

CCSS.RI.11-12.3

CCSS.RI.11-12.5

CCSS.RI.8.3

CCSS.RI.9-10.3

CCSS.RI.9-10.5

How does a buffer work based on the Common-Ion Effect?

• It increases the [H3O+] in the solution

• It decreases the pH of the solution

• It lessens the change in [H3O+] when a strong acid or base is added

• It has no effect on the equilibrium

What is the shift in an equilibrium caused by the addition or removal of one of the species participating in the equilibrium known as?

• Charles's Law

• Avogadro's Law

• Boyle's Law

• Le Chatelier's Principle

In a buffer solution, what is the relation between a weak acid (HA) and its conjugate base (A-) concentrations for the highest buffer capacity?

• [HA] = 2[A-]

• [HA] = [A-]

• [HA] = 0.5[A-]

• [HA] = 4[A-]

What is the pH range over which a buffer acts effectively known as?

• Buffer Range

• Buffer Effectiveness

• Buffer Limit

• Buffer Capacity

Which acid is the best choice to make a buffer solution with a pH of 2.0 based on the given pKa values?

• Chlorous acid (pKa = 1.95)

• Hydrochloric acid (pKa = 6.0)

• Acetic acid (pKa = 4.74)

• Formic acid (pKa = 3.74)

What is the effect of adding a strong base to a buffered solution?

• The pH remains constant

• The pH becomes neutral

• The pH increases slightly

• The pH decreases significantly

What is the purpose of a buffer solution?

• To increase the impact of external forces

• To create a highly acidic environment

• To maintain a stable pH when a strong acid or base is added

• To neutralize all acids and bases

What is the relation between buffer capacity and the concentration of buffer components?

• Higher concentration leads to higher buffer capacity

• No relation between concentration and buffer capacity

• Lower concentration leads to higher buffer capacity

• Higher concentration leads to lower buffer capacity

What is the pH of a buffer solution prepared from 60.0 mL of 0.100 M NH3 and 40.0 mL of 0.100 M NH4Cl? (Given Kb for NH3 is 1.8x10^-5)

• pH = 7.00

• pH = 4.57

• pH = 5.50

• pH = 9.43