Question

To determine the amount of hydrochloric acid present in the whole of the given solution

by conductometric titration using standard sodium hydroxide solution of 0.2 N.
​

Answer 1

Explanation:

Carrying out acid-base titration using a pH meter. Carrying ... present in a standard solution is known as titration. ... Calculate the amount of NaOH and Na2CO3 present in a litre of the given solution in g/ L.

Answer 2

Answer:

Acid-base reactions are of great practical importance in analysis, not only because of their use in titrating a large

number of inorganic and organic substances, but also because the hydrogen ion concentration of a solution often is of

great importance in controlling reactions.

Titration :

The process of determining the volume of a given solution of a reagent equivalent to the amount of another reactant

present in a standard solution is known as titration.

Equivalent Weight of Acids and Bases :

The equivalent weight of an acid is that weight which yields one mole of hydrogen ions in the reaction employed

whereas the equivalent weight of a base is that weight which reacts with one mole of hydrogen ions in the reaction.

Normal solution :

A solution containing one equivalent weight of solute per litre of solution.

Equivalence Point :

When the number of equivalents of acid (respectively base) added is equal to the number of equivalents of base

(respectively acid) taken initially, we have reached the equivalence point.

Acid-Base Indicators :

Weak organic acids or bases having different colours for their dissociated or undissociated forms e.g., phenol red which

is yellow in colour in its undissociated form in acidic solution and red in its dissociated form in basic solution constitute

these indicators.

Name of indicator Colour in acid solution Colour in basic solution pH range

Methyl Orange Red Orange – yellow 3.1 – 4.6

Bromophenol Blue Yellow Blue – violet 3.0 – 4.6

Methyl Red Red Yellow 4.2 – 6.3

Bromothymol Blue Yellow Blue 6.0 – 7.6

Thymol Blue Yellow Blue 8.0 – 9.6

Phenolphthalein Colourless Red 8.0 – 9.8

Thymolphthalein Colourless Blue 9.4 – 10.6

<>Table 38.1 Some acid-base indicators, their colour changes and pH range:

Explanation:

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