   # It took 25.06 ± 0.05 mL of a sodium hydroxide solution to titrate a 0.4016-g sample of KHP (see Exercise 79). Calculate the concentration and uncertainty in the concentration of the sodium hydroxide solution. (See Appendix 1.5.) Neglect any uncertainty in the mass. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 6, Problem 141CP
Textbook Problem
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## It took 25.06 ± 0.05 mL of a sodium hydroxide solution to titrate a 0.4016-g sample of KHP (see Exercise 79). Calculate the concentration and uncertainty in the concentration of the sodium hydroxide solution. (See Appendix 1.5.) Neglect any uncertainty in the mass.

Interpretation Introduction

Interpretation: The concentration and its uncertainty have to be calculated.

Concept introduction: Concentration of a solution can be defined in terms as moles of solute (in grams) to the volume of solution (in litres). The concentration of solution can be calculated by,

Concentration(inM)=Moles ofsolute(ing)Volumeofsolution(inL)

### Explanation of Solution

Explanation

VolumeofNaOHsolution=25.06±0.05mLMassofsample=0.4016g

The mass of the sample (KHP) and volume of solution is recorded as shown above.

To calculate the moles of KHP

MolesofKHP=0.40161mol204.22g=1.967×10-3molKHP

The solution of NaOH contains 1.967×10-3mol because 1 mole of NaOH completely reacts with 1 mole of KHP .

The moles of KHP used are calculated by plugging in the values of mass of the sample to molar mass of KHP . The moles of KHP contained in the NaOH solution is found to be 1.967×10-3mol .

To calculate the concentration and its uncertainty

MolarityofNaOH=1

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