   Chapter 17, Problem 32PS

Chapter
Section
Textbook Problem

Without doing detailed calculations, sketch the curve for the titration of 50 mL of 0.050 M pyridine, C6H5N (a weak base), with 0.10 M HCl. Indicate the approximate pH at the beginning of the titration and at the equivalence point. What is the total solution volume at the equivalence point?

Interpretation Introduction

Interpretation:

The curve for titration of 50 mL of 0.050 M  pyridine, C5H5N with 0.10 M HCl has to be sketched. The approximate pH at the beginning of the titration and at a equivalence point has to be indicated. And the total solution volume at the equivalence point has to be determined.

Concept introduction:

A titration is one of the most useful ways of determining accurately the quantity of an acid , a base or some other substances in a mixture.

The pH at the equivalence point of a strong acid –strong base titration is 7.

A weak acid titrated with a strong base leads to a pH > 7 at the equivalence point.

A weak base titrated with a strong acid leads to pH < 7 at the equivalence point. Indicators:

A chemical substances which gives a visible change  in the titration.

Some important indicators are as follow. Explanation

Pyridine is a weak base , the estimated pH value of the solution is about pH = 9 from the exponent of its Kb value (Kb=1.4×109).

Here, we are using for titration basic solution versus acidic solution. Therefore, acidic solution will be acidic at high concentrations.

The pyridine reacts with hydrogen chloride to form pyridinium chloride. It is a weak acid. Then the solution will be acidic. So the pH can be estimated as pH = 5

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