 # Calculate the base-ionization constants for CN − and CO 3 2− . Which ion is the stronger base? ### General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
Publisher: Cengage Learning
ISBN: 9781305580343 ### General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
Publisher: Cengage Learning
ISBN: 9781305580343

#### Solutions

Chapter
Section
Chapter 16, Problem 16.99QP
Textbook Problem

## Calculate the base-ionization constants for CN− and CO32−. Which ion is the stronger base?

Expert Solution
Interpretation Introduction

Interpretation:

The base ionization constants for CN and CO32 ions has to be calculated and the stronger base among them has to be identified

Concept Introduction:

Relationship between Ka and Kb :

Ka × Kb = Kw

Strength of Base based on Kb value:

• Larger the Kb value; stronger the base is.
• Smaller the Kb value; weaker the base is.

### Explanation of Solution

To Calculate: The base ionization constants for CN and CO32 ions

Base ionization constant for CN :

The hydrolysis of CN ion is as follows,

CN + H2O HCN + OH

The acid ionization constant of HCN is 4.9×1010

The base ionization constant of CN is calculated as follows,

Kb =KwKa =1.0×10144.9×1010 =2.04×105

Therefore, the base ionization constant of CN ion is 2.0×105

Base ionization constant for CO32 :

The hydrolysis of CO32 ion is as follows,

CO32 + H2O HCO3 + OH

The HCO3 ion is the conjugate acid of CO32

The ionization constant (Ka2) of HCO3 is 4

### Want to see the full answer?

Check out a sample textbook solution.See solution

### Want to see this answer and more?

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

See solution 