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Question

What will be the normality of the solution obtained by mixing 100 mL of 0.2 M H2SO4​ with 100 mL of 0.2 M NaOH ?

A
0.05 N
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B
0.01 N
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C
0.5 N
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D
0.1 N
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Solution

The correct option is D 0.1 N
Normality=Molarity×nf
H2SO4 is dibasic acid nfactor=2
n-factor for NaOH=1, as it is a monoacidic base.
N1 of H2SO4=0.2×2=0.4
N2 of NaOH=0.2×1=0.2
The required formula is -
N1V1N2V2=N3V3

where, V1​ and V2​ are the volumes of H2SO4 and NaOH respectively.
Given , V1=V2=100 mL
V3=100+100=200 mL
Where, N3​ and V3​ are the normality & volume of the final solution.

(0.4×100)(0.2×100)=N3×(200)N3=20200N3=0.1 N
The normality of solution obtained is 0.1 N.


Titrations :

Types of titrations :

1. Acid - base titrations 2. Redox titrations

Equivalence point is the point where:

No. of equivalent of the analyte = No. of equivalent of the titrant

1. Analyte: Solution with unknown concentration

2. Titrant: Solution with known concentration

Redox titration :

In this titration, one oxidizing agent (O.A.) reacts with one reducing agent (R.A.).

O.A+R.Aproducts

At the equivalence point :

Equivalence of O.A. = Equivalence of R.A


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