Multiple Choice
Calculate the pH value for a buffer solution prepared by adding 1.0 mL of a 0.10M acetic acid solution to 20 mL of a 0.10M sodium acetate solution. (Ka = 1.7 × 10⁻⁵)
18. Aqueous Equilibrium
Intro to Buffers
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Which component of the acetic acid buffer pair would react with added NaOH?
A
Acetic acid (CH3COOH)
B
Sodium ion (Na+)
C
Acetate ion (CH3COO-)
D
Water (H2O)
Verified step by step guidance1
Identify the components of the acetic acid buffer system: acetic acid (CH3COOH) and acetate ion (CH3COO-).
Understand that a buffer solution resists changes in pH upon the addition of small amounts of acid or base.
Recognize that when NaOH, a strong base, is added to the buffer, it will react with the acidic component of the buffer.
Determine that the acidic component in the acetic acid buffer is the acetic acid (CH3COOH), which can donate a proton (H+) to neutralize the added OH- from NaOH.
Conclude that the acetate ion (CH3COO-) is the component that will react with the added NaOH, as it is the conjugate base that can accept a proton from the acetic acid, maintaining the buffer's pH.
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