Question

Explain bronsted lowry concept of acid and base with an example

Answer 1

The Bronsted-Lowry definition of acids and bases is pretty simple. An acid is a proton donor, and a base is a proton acceptor. In the example of ammonia dissolving in water (NH3 + H2O = NH4+ + OH-), the water donates a proton, so it is the acid. ... The hydroxide ion is accepting the proton and is called a conjugate base.

Answer 2

Explanation:

According to the Bronsted-Lowry conjugate acid-base theory, an acid is defined as a substance which looses donates protons and thus forming conjugate base and a base is defined as a substance which accepts protons and thus forming conjugate acid.

For the given chemical equation:

$H_3BO_3(aq.)+HS^-(aq.)\rightarrow H_2BO_3^-(aq.)+H_2S(aq.)$

Here, is loosing a proton, thus it is considered as a brønsted-lowry acid and after losing a proton, it forms which is a conjugate base.

$HS^-$  is gaining a proton, thus it is considered as a brønsted-lowry base and after gaining a proton, it forms $H_2S$ which is a conjugate acid.

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