   # What is the pH of a buffer solution prepared from 5.15 g of NH 4 NO 3 and 0.10 L of 0.15 M NH 3 ? What is the new pH if the solution is diluted with pure water to a volume of 5.00 × 10 2 mL? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 17, Problem 85GQ
Textbook Problem
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## What is the pH of a buffer solution prepared from 5.15 g of NH4NO3 and 0.10 L of 0.15 M NH3? What is the new pH if the solution is diluted with pure water to a volume of 5.00 × 102 mL?

Interpretation Introduction

Interpretation:

For the buffer solution which is prepared by adding 5.15 g of ammonium nitrate in 0.10 L of 0.15 M NH3 the pH of the buffer solution and after the dilution volume of buffer solution to 5.0×102 mL has to be calculated.

Concept introduction:

The Henderson-Hasselbalch equation relates pOH of a buffer with pKb of base, concentration of conjugate acid and concentration of base. The expression is written as,

pOH=pKb+log[conjugateacid][base] (1)

This equation shows that pOH of buffer solution is controlled by two major factors. First, is strength of the base which can be expressed on terms of pKb and second, the relative concentration of base and its conjugate acid at equilibrium.

The pH value is calculated by expression, pH + pOH = 14.

### Explanation of Solution

• The calculation of pH is done by using Henderson-Hasselbalch equation.

Given:

Refer to table 16.2 in the textbook for the value of Kb.

The value of Kb for NH3 is 1.8×105.

The pKb value is calculated as follows;

pKb=log(Kb)

Substitute 1.8×105 for Kb.

pKb=log(1.8×105)=4.74

Therefore, pKb value of NH3 is 4.74.

The initial concentration of NH3 is 0.15 molL1.

The initial moles of NH4NO3 is 0.0643 mol.

The volume of the buffer solution is 0.10 L.

The concentration of NH4NO3 is calculated as follows;

Molarity=Number of molesvolume of solvent (2)

Substitute 0.0643 mol for number of moles and 0.10 L for volume of solvent in equation (2).

Molarity=0.0643 mol0.10 L=0.643 molL1

Therefore, the concentration of NH4NO3 is 0.643 molL1.

The value of pH is calculated by using equation (1).

pOH=pKb+log[conjugateacid][base]

Substitute 4.74 for pKb, 0.643 for [conjugate acid], 0.15 for [base].

pOH=4.74+log(0.643)(0.15)=4.74+log(4.2866)=4.74+0.63=5.37

Therefore, pOH value of the buffer solution is 5.37.

The pH value is calculated by using expression,

pH + pOH = 14

Rearrange for pH

pH  = 14pOH

Substitute 5.37 for pOH

pH  = 145.378.63

Therefore value of pH for the buffer solution is 8.63.

Calculation of pH for the buffer solution when it is diluted to 5×102 mL or 0.500 L.

After dilution concentration of ammonia and ammonium nitrate will change as volume of the buffer increases.

Concentration of ammonia after dilution is calculated by using the following expression.

C1V1=C2V2

Here,

• C1 is the initial concentration of ammonia

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