Chemistry
Chemistry
13th Edition
ISBN: 9781259911156
Author: Raymond Chang Dr., Jason Overby Professor
Publisher: McGraw-Hill Education
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Textbook Question
Chapter 15, Problem 15.66QP

Calculate the concentrations of H+, HCO 3 , and CO 3 2 in a 0.025 M H2CO3 solution.

Expert Solution & Answer
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Interpretation Introduction

Interpretation:

The concentrations of HCO3-,CO32andH+ ions in a 0.025 M H2CO3 solution has to be calculated.

Concept Information:

Acid ionization constant Ka:

Acids ionize in water.  Strong acids ionize completely whereas weak acids ionize to some limited extent.

The degree to which a weak acid ionizes depends on the concentration of the acid and the equilibrium constant for the ionization.

The ionization of a weak acid HA can be given as follows,

HA(aq)H+(aq)+A-(aq)

The equilibrium expression for the above reaction is given below.

Ka=[H+][A-][HA]

Where,

Ka is acid ionization constant,

[H+] is concentration of hydrogen ion

[A-] is concentration of acid anion

[HA] is concentration of the acid

To Calculate: The concentrations of HCO3-,CO32andH+ ions in a 0.25 M H2CO3 solution

Answer to Problem 15.66QP

  • The concentration of HCO3- ion is 1.0×104 M
  • The concentration of CO32- ion is 4.8×1011 M
  • The concentration of H+ ion is 1.0×104 M

Explanation of Solution

Record the given datas

The concentration of H2CO3 solution is 0.025 M

H2CO3 is a weak acid with a concentration of 0.025 M. Using the ionization constant for H2CO3 the concentration of HCO3-,CO32andH+  can be calculated

First ionisation of H2CO3

Calculation of [HCO3]and[H+]

H2CO3 is a weak acid. The first ionization stage of H2CO3 is as follows,

H2CO3(aq)H+(aq)+HCO3(aq)

The concentration of all the species before and after ionization can be represented as follows,

 H2CO3(aq)H+(aq)+HCO3-(aq)
Initial (M)

0.025

x

0.025x

0.000.00
Change (M)+x+x
Equilibrium (M)+x+x

The acid ionization constant H2CO3 of is 1.0×104M

Ka=[H+][HCO3-][H2CO3-]4.2×107=x2(0.025x)x20.025x=1.0×104M

Therefore, the concentration of [HCO3]=[H+]=1.0×104M

Second stage ionization of H2CO3

Consider the second stage of ionization HCO3 is a weak acid. Set up a table showing the concentrations for the second ionization stage.

Let y be the change in concentration.

Note the initial concentration of H+ is 1.0×104M from the first ionization.

 HCO3(aq)H+(aq)+CO32(aq)
Initial (M)

1.0×104

y

1.0×104y

0.000.00
Change (M)+y+y
Equilibrium (M)1.0×104+yy

Calculation of [CO32-] ion concentration

Write the ionization constant Ka . Then, solve for y.

The Ka for HCO3 is 4.8×10-11

Ka=[H+][CO32-][HCO3-]4.8×1011=[(1.0×104)+y](y)1.0×104y(1.0×104)(y)1.0×104y=4.8×1011M

Since HCO3 is a very weak acid, there is little ionization at this stage.

Therefore,  [CO32-] ion concentration is 4.8×1011M

Conclusion

The concentrations of HCO3-,CO32andH+ ions in a 0.025 M H2CO3 solution was calculated.

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Chapter 15 Solutions

Chemistry

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