Question

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

Answer 1

The equation that shows ${\text{HCO}}_3^ -$  acts as base with ${\text{H}}{{\text{S}}^ - }$  as an acid is $\boxed{{\text{HCO}}_3^ - +{\text{H}}{{\text{S}}^ - }\rightleftharpoons{{\text{H}}_2}{\text{C}}{{\text{O}}_3}+{{\text{S}}^{2 - }}}$

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, ${\text{HN}}{{\text{O}}_3}$ and ${{\text{H}}_2}{\text{S}}{{\text{O}}_4}$  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 ${\text{N}}{{\text{H}}_3}$  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 ${\text{B}}{{\text{F}}_3}$ , ${\text{S}}{{\text{O}}_3}$  while ${{\text{H}}_2}{\text{O}}$  and ROH are the examples of Lewis base.

The required equation is as follows:

${\text{HCO}}_3^ - +{\text{H}}{{\text{S}}^ - }\rightleftharpoons{{\text{H}}_2}{\text{C}}{{\text{O}}_3}+{{\text{S}}^{2 - }}$

Here, ${\mathbf{HCO}}_{\mathbf{3}}^{\mathbf{ - }}$  accepts a proton and becomes ${{\text{H}}_2}{\text{C}}{{\text{O}}_3}$  whereas ${\mathbf{H}}{{\mathbf{S}}^{\mathbf{ - }}}$  donates a proton and forms ${{\text{S}}^{2 - }}$. 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 brainly.com/question/1550328

2. Reason for the acidic and basic nature of amino acid. brainly.com/question/5050077

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.

Answer 2

Answer:  $HCO_{3}^{-}+ HS^{-}\rightleftharpoons H_{2}CO_{3} + S^2{-}$

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.

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

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.