Question

Which are the Brønsted–Lowry acids in the following equilibrium?Which are the Brønsted–Lowry acids in the following equilibrium? CH3COOH(aq) + NaOH(l)⇌ NaCH3COO(aq) + H2O(l)CH3COOH(aq) + NaOH(l)⇌ NaCH3COO(aq) + H2O(l)

Select one:

a. CH3COO–and OH––

b. H2O and OH–

c. H2O, CH3COOH, and OH–

d. CH3COO–and CH3COOH

e. H2O and CH3COOH

Answer 1

Ans. Given reaction: CH₃COOH(aq) + NaOH(aq) ---------> NaCH₃COO^-(aq) + H₂O

# A Bronsted-Lowery acid is a chemical species that donates a proton (H⁺). A Bronsted-Lowery base is a chemical species that accepts a proton (H⁺)

# In the given reaction, CH₃COOH acts as Bronsted-Lowry acid. However, due to reaction with strong base (NaOH), all of CH3COOH would be present in form of CH₃COO^-. Since there is no more acid (CH₃COOH) in the reaction mixture, no equilibrium of Bronsted-Lowry acid would be established.

# The conjugate base in above reaction, NaCH₃COO^-, would accept a proton from H₂O as follow-

            NaCH₃COO^-(aq) + H₂O(l) <--------> NaCH₃COOH(aq) + OH^-

In the above reaction, H₂O acts as weak acid (weak Bronsted-Lowry acid) and is in equilibrium with its conjugate base OH^-.

Therefore, for the given reaction, the Bronsted-Lowry acid H₂O is in equilibrium with its conjugate base OH^-.

# So, correct option is- B. H₂O and OH^-