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Question

What will be the normality of the solution obtained by mixing 50 mL of 0.2 M H2SO4​ with 50 mL of 0.1 N Ca(OH)2 ?

A
0.20 N
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B
0.20 N
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C
0.15 N
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D
0.10 N
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Solution

The correct option is C 0.15 N
Normality=Molarity×nf
H2SO4 is dibasic acid nfactor=2
N1 of H2SO4=0.2×2=0.4 N
N2 of Ca(OH)2=0.1 N

The required formula is -
N1V1N2V2=N3V3

where, V1​ and V2​ are the volumes of H2SO4 and Ca(OH)2 respectively.
Given , V1=V2=50 mL
V3=50+50=100 mL
Where, N3​ and V3​ are the normality & volume of the final solution.

(0.4×50)(0.1×50)=N3×(100)N3=15100N3=0.15 N
The normality of the resultant acidic solution is 0.15 N.


Important list of Reactions and Half Reactions :

Cr2O27Cr3+

MnO4Mn2+(Acidic)

MnO4MnO2(Basic/Neutral)

MnO4MnO24(HighlyBasic)

IO3I

MnO2Mn2+(Acidic)

I2I

ClOCl

H2O2H2O

NO3NO2

NO3NO2

NO3NO

NO3N2O

NO3NH+4

\(O_3 \longrightarrow O_2 + O^{2-}

Fe2+Fe3+

Sn3+Sn3+

S2O23S4O26

S2S

NO2NO3

H2O2O2

C2O24CO2

ZnZnO2(Basic)


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