Write an equation to show how hco3− can act as a base with hs− acting as an acid.

The equation that shows  acts as base with  as an acid is

Further Explanation:

Acids and bases can be defined in many ways based on different theories, which are as follows:

1. Arrhenius theory: According to this theory, acid is defined as the one which produces hydrogen or hydronium ions in a solution, while the base is defined as the one which produces hydroxide ions in a solution. Examples of Arrhenius acids include HBr, and  while NaOH and KOH are examples of Arrhenius bases.

2. Bronsted-Lowry theory: According to this theory, the acid in the reaction donates a proton while a base is one that accepts a proton. HCl acts as Bronsted acid while  is a Bronsted base.

3. Lewis theory: According to this theory, an acid accepts a pair of electrons to electron-rich species while a base donates electrons to electron-deficient species in the reaction. Examples of Lewis acids are ,  while  and ROH are the examples of Lewis base.

The required equation is as follows:

Here,  accepts a proton and becomes  whereas  donates a proton and forms . According to Bronsted-Lowry theory, any species that accepts proton is called base while the one that donates proton acts as an acid.  

Learn more:

1. The reason for the acidity of water link

2. Reason for the acidic and basic nature of amino acid. link

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Chemical reaction and equation

Keywords: acid, base, electrons, protons, Arrhenius theory, Lewis theory, Bronsted-Lowry theory, hydrogen, hydronium ion, hydroxide ion, HCO3-, HS-, S2-, H2CO3.