Calculate the equilibrium constant, Kc, of the reaction: HCO3-(aq) + HCO3-(aq) ↔ H2CO3(aq) + CO32- , Kc = ? Based on your result, do you expect this reaction to occur in the left-to-right direction? Complete the Kai expression for H₂CO3 in an aqueous solution.Kal=4.45 × 10-7=[H3O+][HCO3][H₂CO3] Complete the K₁2 expression for H₂CO3 in an aqueous solution.Ka2 = 4.69 × 10-11=[CO-][HCO3][H3O+]

An equilibrium chemical reaction is given as follows: ...(i)The equilibrium constant can be defined…

Answered: Calculate the equilibrium constant, Kc,…

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter8: Acids And Bases

Section: Chapter Questions

Problem 8.90P

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Related questions

Question

Calculate the equilibrium constant, Kc, of the reaction:

HCO3-(aq) + HCO3-(aq) ↔ H2CO3(aq) + CO32- , Kc = ?

Based on your result, do you expect this reaction to occur in the left-to-right direction?

Complete the Kai expression for H₂CO3 in an aqueous solution.
Kal
=
4.45 × 10-7
=
[H3O+]
[HCO3]
[H₂CO3]

Complete the K₁2 expression for H₂CO3 in an aqueous solution.
Ka2 = 4.69 × 10-11
=
[CO-]
[HCO3]
[H3O+]

Expert Solution

Step 1: Given information:

An equilibrium chemical reaction is given as follows:

$H C O subscript 3 to the power of minus space left parenthesis a q right parenthesis space plus space H C O subscript 3 to the power of minus space left parenthesis a q right parenthesis space left right arrow space H subscript 2 C O subscript 3 space left parenthesis a q right parenthesis space plus space C O subscript 3 to the power of 2 minus end exponent space left parenthesis a q right parenthesis$ ...(i)

The equilibrium constant can be defined as the ratio of the product of the equilibrium molar concentrations of products and the product of the equilibrium molar concentrations of reactants, with the each concentration term raised to an exponent equal to the stoichiometric coefficient.

We have to determine the equilibrium constant, K_c for the above equilibrium.

The first acid dissociation constant, K_a1 for H₂CO₃ is given as $4.45 space cross times space 10 to the power of negative 7 end exponent$ .

The second acid dissociation constant, K_a2 for H₂CO₃ is given as $4.69 space cross times space 10 to the power of negative 11 end exponent$ .

H₂CO₃is a weak diprotic acid and its dissociation takes place in two steps.