Explanation N H 3 is a weak base and its conjugate acid is N H 4 + . The required equilibrium is given below. N H 3 ( a q ) + H 2 O ( l ) ⇌ O H = ( a q ) + N H 4 + ( a q ) K b = [ O H − ] [ N H 4 + ] [ N H 3 ] = 1.8 × 10 − 5 Given that, the buffer contains 0.040 M N H 4 C l ( a q ) and 0.030 M N H 3 ( a q ) . The equilibrium concentration of O H − ions can be calculated as shown below. K b = [ O H − ] [ N H 4 + ] [ N H 3 ] = 1

Chemical Principles: The Quest for Insight

7th Edition

ISBN: 9781464183959

Author: Peter Atkins, Loretta Jones, Leroy Laverman

Publisher: W. H. Freeman

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Chapter 6, Problem 6G.1BST

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Interpretation:

The pH of a buffer solution that is 0.040 M NH4Cl(aq) and 0.030 M NH3(aq) has to be calculated.

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Chapter 6, Problem 6G.1AST

Chapter 6, Problem 6G.2AST

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Chapter 6 Solutions

Chemical Principles: The Quest for Insight

Ch. 6 - Prob. 6A.1AST Ch. 6 - Prob. 6A.1BST Ch. 6 - Prob. 6A.2AST Ch. 6 - Prob. 6A.2BST Ch. 6 - Prob. 6A.3AST Ch. 6 - Prob. 6A.3BST Ch. 6 - Prob. 6A.1E Ch. 6 - Prob. 6A.2E Ch. 6 - Prob. 6A.3E Ch. 6 - Prob. 6A.4E

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The p H of a buffer solution that is 0.040 M N H 4 C l ( a q ) and 0.030 M N H 3 ( a q ) has to be calculated.

Solution Summary: The author calculates the pH of a buffer solution that contains 0.040MTextNH_4Cl(aq) and 0.030

Interpretation:

The pH of a buffer solution that is 0.040 M NH4Cl(aq) and 0.030 M NH3(aq) has to be calculated.

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Chapter 6 Solutions

The p H of a buffer solution that is 0.040 M N H 4 C l ( a q ) and 0.030 M N H 3 ( a q ) has to be calculated.

Solution Summary: The author calculates the pH of a buffer solution that contains 0.040MTextNH_4Cl(aq) and 0.030

Interpretation: The pH of a buffer solution that is 0.040 M NH4Cl(aq) and 0.030 M NH3(aq) has to be calculated.

Want to see the full answer?

Chapter 6 Solutions

Interpretation:

The pH of a buffer solution that is 0.040 M NH4Cl(aq) and 0.030 M NH3(aq) has to be calculated.