Question

Conjugate base for Bronsted acids $H_2O$ and $HF$ are:

• A. $OH^-$ and $F^-$, respectively
• B. $H_3O^+$ and $H_2F^+$, respectively
• C. $OH^-$ and $H_2F^+$, respectively
• D. $H_3O^+$ and $F^-$ respectively

Answer 1

The Correct Option is A

To solve this problem, we need to understand the concept of Bronsted acids and their conjugate bases.

A Bronsted acid is a substance that can donate a proton (H^+). When a Bronsted acid donates a proton, it forms its conjugate base. The conjugate base is the species that remains after the acid has donated a proton.

1. Conjugate Base of H_2O:
   • Water (H_2O) can act as an acid by donating a proton:
     H_2O \rightarrow OH^- + H^+
   • Therefore, the conjugate base of H_2O is OH^−.
2. Conjugate Base of HF:
   • Hydrofluoric acid (HF) can also donate a proton:
     HF \rightarrow F^- + H^+
   • Therefore, the conjugate base of HF is F^−.

Given the choices, the correct conjugate bases for H_2O and HF are OH^− and F^−, respectively.

Correct Answer: OH^− and F^−, respectively.