A buffer solution is made up of acetic acid (CH3COOH) and sodium acetate (NaCH3COO). The major equilibria in the buffer system a

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A buffer solution is made up of acetic acid (CH3COOH) and sodium acetate (NaCH3COO). The major equilibria in the buffer system a

re represented above. Which of the following equilibria could be used to support the claim that the addition of a small amount of NaOH to the buffer will result in only a very small change in pH?
CH3COOH (aq) + H2O → H3O+ (aq) + CH3COO- (aq)
CH3COO- (aq) + H2O → CH3COOH (aq) + OH-
2H2O (i) → H2O + OH-
a. CH3COOH(aq) + CH3COO- (aq) → CH3COO- (aq) + CH3COOH(aq).
b. CH3COOH(aq) + OH (aq) → 3CH3COO (aq) + H2O(1).
c. H3O+ (aq) + OH(aq) → 2H2O(1).
d. CH3COOH(aq) + H2O(1) → H30+ (aq) + CH3COO (aq).

Chemistry

1 answer:

katrin [286] · Answer 1 · 2023-03-13T15:52:06+03:00

The equilibria showing how the acetate buffer adjusts to addition of a small amount of NaOH is:

CH3COOH(aq) + H2O(1) → H30+ (aq) + CH3COO (aq)

<h3>What is a buffer?</h3>

A buffer is a solution which resists changes to its pH when small amounts of strong base or acid is added to it.

Buffers are made from solutions of weak acids and their salts or weak bases and their salts.

The equilibria showing how a buffer made from acetic acid and sodium acetate (NaCH3COO) adjusts to addition of a small amount of NaOH is as follows:

CH3COOH(aq) + H2O(1) → H30+ (aq) + CH3COO (aq)

Addition of NaOH, a strong base will neutralize the hydronium ion, causing the acetic acid ionization equilibrium to shift to the right to produce more of the acetate ion, the conjugate base.

Learn more about acetate buffer at: brainly.com/question/17490438