Both HCO{3}− and HS− are amphoteric. Write an equation to show how each substance can...

William Burnett

William Burnett

Answered

2022-01-12

Both HCO{3} and HS are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.

Answer & Explanation

Ronnie Schechter

Ronnie Schechter

Expert

2022-01-13Added 27 answers

HCO3(ag)+HS(ag)CO32(ag)+H2S(aq)
Let HCO{3} be a Br nsted-Lowry acid and let HS be a Br nsted-Lowry base. The conjugate base of the acid is then determined by removing an H atom and
a unit of positive charge. The conjugate acid of the base is then determined by adding an H atom anda unit of positive charge.
HCO3(ag)+HS(ag)H2CO3(ag)+S2(aq)
Let HCO{3} be a ​​​​​​​Br nsted-Lowry base and let HS
be a Br nsted-Lowry acid. The conjugate acid of the
base is then determined by adding an H atom anda unit of positive charge. The conjugate base of the acid is then determined by removing an H atom and a unit of positive charge.

soanooooo40

soanooooo40

Expert

2022-01-14Added 35 answers

Explanation:
According to Bronsted and Lowry an acid is a proton donor and base is a proton acceptor.
Therefore, the equation for the reaction will be as follows.
HCO3+HS=H2CO3+S2t
Here, HCO{3} acts as a base as it is accepting a proton and HS acts as an acid because it is donating a proton.

Do you have a similar question?

Recalculate according to your conditions!

Ask your question.
Get your answer.

Let our experts help you. Answer in as fast as 15 minutes.

Didn't find what you were looking for?