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Standard XII

Chemistry

Introduction to Oxidation and Reduction

Two drops of ...

Question

Two drops of methyl ogrange is added to $20.0 m L$ of $0.05 M$ ${N a}_{2} {C O}_{3}$ solution and this is titrated against $H C l$ taken in a burette. Light pinkish red colour was obtained when the volume of the acid added was $23.5 m L$ . The concentration of the acid was?

0.100 M

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0.150 M

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0.085 M

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0.095 M

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Solution

The correct option is C $0.085 M$
Given
Molarity of $N a_{2} C O_{3}$ =0.05M
Volume of $N a_{2} C O_{3}$ =20ml
Volume of $H C l$ = 23.5ml
Molarity of $H C l$ = ?
Solution
$N a_{2} C O_{3} + 2 H C l = 2 N a C l + H_{2} O + C O_{2}$
As 1 mole of base is reacting with 2 mole of acid
Hence
Using volumetric principle of titration
$\frac{m o l e s o f a c i d}{m o l e s o f b a s e} = \frac{2}{1}$

Moles of acid = $M_{H C l} * V_{H C l}$

Moles of base= $M_{N a_{2} C O_{3}} * V_{N a_{2} C O_{3}}$

$\frac{M * 23.5}{0.05 * 20} = \frac{2}{1}$

$M = 0.085 M$

The correct option is C

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Two drops of methyl ogrange is added to 20.0mL of 0.05M Na2CO3 solution and this is titrated against HCl taken in a burette. Light pinkish red colour was obtained when the volume of the acid added was 23.5mL. The concentration of the acid was?

Two drops of methyl ogrange is added to $20.0 m L$ of $0.05 M$ ${N a}_{2} {C O}_{3}$ solution and this is titrated against $H C l$ taken in a burette. Light pinkish red colour was obtained when the volume of the acid added was $23.5 m L$ . The concentration of the acid was?