Question 1

Which of the following best describes the function of a buffer solution in the human body?

Accepted Answer

A buffer solution maintains the pH by neutralizing small amounts of added acid or base.

Question 2

Which combination below will create a buffer solution?

Accepted Answer

H$$_2CO$_3$$ and NaHCO$$_3$$

Question 3

What happens to the pH of pure water when a small amount of acid is added?

Accepted Answer

The pH decreases drastically.

Question 4

Which equation represents the neutralization of a base by acetic acid in a buffer?

Accepted Answer

$$\mathrm{HC_2H_3O_2} + \mathrm{OH^-} \rightarrow \mathrm{C_2H_3O_2^-} + \mathrm{H_2O}$$

Question 5

A buffer solution contains equal concentrations of acetic acid and sodium acetate. What will happen if a small amount of H$$_3O$^+ is $$added?

Accepted Answer

The acetate ion will neutralize the added H$$_3O$^+$$, maintaining the pH.

Question 6

Which of the following is NOT a property of a buffer solution?

Accepted Answer

Contains only strong acids and strong bases.

Question 7

In the buffer system of acetic acid and sodium acetate, what is the role of the acetate ion ($$\mathrm{C_2H_3O_2^-}$$)?

Accepted Answer

To neutralize added H$$_3O$^+$$ ions.

Question 8

A student adds a small amount of NaOH to a buffer solution containing acetic acid and sodium acetate. What is the primary reaction that occurs?

Accepted Answer

$$\mathrm{HC_2H_3O_2}$$ neutralizes the added OH$$^-$$, forming $$\mathrm{C_2H_3O_2^-}$$ and $$\mathrm{H_2O}.$$

Question 9

Which of the following statements about buffers is TRUE?

Accepted Answer

Buffers are important for maintaining pH in blood and cellular processes.

Question 10

If a buffer solution is overwhelmed by a large amount of acid or base, what will happen?

Accepted Answer

The pH will change drastically once the buffer capacity is exceeded.

Question 11

Which equation represents the neutralization of an acid by the conjugate base in a buffer?

Accepted Answer

$$\mathrm{C_2H_3O_2^-} + \mathrm{H_3O^+} \rightarrow \mathrm{HC_2H_3O_2} + \mathrm{H_2O}$$

Question 12

Which of the following best explains why buffers are important in blood?

Accepted Answer

Buffers maintain a pH close to 7.4, which is necessary for proper cellular function and oxygen uptake.

Question 13

Which of the following is a common misconception about buffer solutions?

Accepted Answer

Buffers are made from strong acids and strong bases.

Question 14

A buffer solution is prepared with acetic acid and sodium acetate. If the concentration of acetic acid is doubled while the concentration of sodium acetate remains the same, what will happen to the buffer's ability to neutralize added OH$$^-$$?

Accepted Answer

The buffer will be more effective at neutralizing OH$$^-.$$

Question 15

Which of the following is the correct formula for calculating pH?

Accepted Answer

$$\mathrm{pH} = -\log[\mathrm{H_3O^+}]$$

Question 16

Which of the following best describes the relationship between reversible reactions and equilibrium in acid-base chemistry?

Accepted Answer

Equilibrium is reached when the rates of the forward and reverse reactions are equal.

Question 17

A buffer solution is made with equal concentrations of a weak acid and its conjugate base. What is the effect on pH if a small amount of base is added?

Accepted Answer

The weak acid neutralizes the base, causing only a slight increase in pH.

Question 18

Which of the following is a real-life example of a buffer system?

Accepted Answer

The combination of H$$_2CO$_3$$ and NaHCO$$_3 in $$blood.

Buffers: Maintaining pH in Acid-Base Equilibrium

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