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Salt of Weak Acid and Weak Base

Indicator V...

Question

Indicator $V$ could be used to find the equivalence point for $0.1 M$ acetic acid and $0.1 M$ ammonium hydroxide solution.

A

True

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B

False

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Solution

The correct option is B False
The indicator $V$ changes its colour formed to yellow in a $p H$ range from $2.8$ to $4.1$ .
Now $0.1 M$ ${C H}_{3} C O O H$ reacts with $0.1 M$ ${N H}_{4} O H$ to form ${C H}_{3} {C O O N H}_{4}$ . The $p H$ will be around $7.0$ (because ${p K}_{a} \approx 4.7$ and ${p K}_{b} \approx 4.7$ ). So the indicator $V$ ( $p H$ $2.8$ to $4.1$ ) can not be used.
Answer will be false.

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Similar questions

Q. Calculate the pH at the equivalence point when a solution of

0.1 M

acetic acid is titrated with a solution of

0.1 M

sodium hydroxide.

K_{a}

for acetic acid

= 1.9 \times 10^{- 5}

Q. For a series of indicators, the colours and pH range over which colour change takes are as follows:

Indicator	Colour change over pH range
U	Yellow to blue pH 0.0 to 1.6
V	Red to yellow pH 2.8 to 4.1
W	Red to yellow pH 4.2 to 5.8
X	Yellow to blue pH 6.0 to 7.7
Y	Colourless to red pH 8.2 to 10.0

Which of the following statements is/are correct?

U

could be used to distinguish between

0.1 M

0.01 M

solution of sulphuric acid.

O H^{-}

concentration at the equivalent point when a solution of

0.1 M

acetic acid is titrated with a solution of

0.1 M

K_{2}

= 1.9 \times 10^{- 3}

Q. No indicator can be used for the titration between formic acid and ammonium hydroxide because:

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