Question

Consider this reaction: HCO3− H2S → H2CO3 HS− Which is the Bronsted-Lowry base? H2S HCO3- HS– H2CO3.

Answer 1

Bronsted Lowry base is the species that accepts or acquires protons from other species of the reaction. $\rm HCO_{3}^{-}$is the Bronsted-Lowry base.

What is a Bronsted-Lowry base?

In an acid-base reaction, the element or the compound capable of obtaining a proton or a hydrogen atom is called a Bronsted-Lowry base.

According to the theory, the base will accept proton and acid will donate an electron. The reaction of the acid and base is shown as,

$\rm HCO_{3}^{-} + H_{2}S \rightarrow H_{2}CO_{3} + HS^{-}$

From the reaction, it can be said that bicarbonate is the Bronsted-Lowry base as the number of hydrogen or protons are increasing in the product.

Therefore, option b. $\rm HCO_{3}^{-}$ is the Bronsted-Lowry base.

Learn more about Bronsted-Lowry base here:

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