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

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22-03-2018
Chemistry

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

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AkshayG AkshayG · Answer 1 · 2019-09-05T14:20:54+02:00

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

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

The required equation is as follows:

[tex]{\text{HCO}}_3^ - +{\text{H}}{{\text{S}}^ - }\rightleftharpoons{{\text{H}}_2}{\text{C}}{{\text{O}}_3}+{{\text{S}}^{2 - }}[/tex]

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

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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.

pstnonsonjoku pstnonsonjoku · Answer 2 · 2021-10-28T19:02:36+02:00

The acid - base reaction between HCO3^- and HS^- is HCO3^-(aq) + HS^-(aq) -------> H2CO3(aq) + S^2-(aq)

According to the Brownstead - Lowry definition of acids and bases, an acid is a substance that donates protons while a base is a substance that accepts protons.

The reaction between HCO3^- and HS^- is an acid base reaction in the Brownstead - Lowry sense of acid base reaction. The reaction occurs as follows; HCO3^-(aq) + HS^-(aq) -------> H2CO3(aq) + S^2-(aq)

HS^- acts as an acid in this reaction because it donates a proton while HCO3^- acts as a base because it accepts a proton according to Brownstead - Lowry definition.

Learn more: https://brainly.com/question/18956703