Question

In the reaction H2CO3 + H 2O ------><-------- HCO 3 − + H 3O +, the Brønsted acids are: H2CO3 and H2O. HCO3− and H2CO3. H2O and H3O+. H3O+ and H2CO3. H2O and HCO3−.

Answer 1

Answer: The bronsted acids for the given reaction are $H_3O^+\text{ and }H_2CO_3$

Explanation:

According to the Bronsted-Lowry conjugate acid-base theory:

• An acid is defined as a substance which looses or donates protons and thus forming conjugate base.
• A base is defined as a substance which accepts protons and thus forming conjugate acid.

For the given chemical equation:

$H_2CO_3+H_2O\rightleftharpoons HCO_3^-+H_3O^+$

For the forward reaction, $H_2CO_3$ looses 1 proton to form $HCO_3^-$ and thus acts as bronsted acid.

For the backward reaction, $H_3O^+$ looses 1 proton to form $H_2O$ and thus acts as bronsted acid

Hence, the bronsted acids for the given reaction are $H_3O^+\text{ and }H_2CO_3$

Answer 2

The bronsted acids for the given reaction are $H_3O^+$ and $H_2CO_3$.

Bronsted-Lowry Theory:

According to the Bronsted-Lowry conjugate acid-base theory:

An acid is characterized as a substance which looses or gives protons and along these lines shaping form base. A base is characterized as a substance which acknowledges protons and accordingly framing form conjugate acid.

From the chemical equation:

$H_2CO_3+H_2O---- > HCO_3^-+H_3O^+$

For the forward reaction, carbonic acid looses 1 proton to form carbonate ion and thus acts as bronsted acid.

For the backward reaction, hydronium ion  looses 1 proton to form water and thus acts as bronsted acid

Hence, the bronsted acids for the given reaction are  $H_3O^+$ and $H_2CO_3$.

Find more information about Bronsted theory here:

brainly.com/question/12916250