Question

Consider this reaction: HCO3− + H2S → H2CO3 + HS−

Which is the Bronsted-Lowry base?

H2S
HCO3-
HS–
H2CO3

Answer 1

Answer: The correct option is $HCO_3^-$

Explanation:

According to the Bronsted Lowry conjugate acid-base pair, an acid is a substance that donates protons and a base is a substance that accepts protons.

From the given options, $HCO_3^-$ represents a Brønsted Lowry base as it is accepting $H^+$ and $H_2S$  represents a Brønsted Lowry acid as it is donating $H^+$.

$HCO_3^-+H^+\rightleftharpoons H_2CO_3$

$H_2S\rightleftharpoons HS^-+H^+$

Answer 2

Answer:

HCO3-

Explanation:

The Bronsted-Lowry acid-base theory states that in a chemical equation, acid is represented by the element that is donating protons within the equation, while the base is the substance that is receiving these protons.

In the case of the chemical equation HCO3− + H2S → H2CO3 + HS−, the element HCO3− is the base, since it is this element that receives readiness that transforms it into H2CO3, while the element H2S is the acid since it is that element that donates protons turning into HS−.