Question

calculate normality and molarity of solution of H2so4 obtained by dissolving 0.49 g of it in 500 if solution
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Answer 1

Answers :-

Molarity = 0.01

Normality = 0.02

Given :-

• Weight (w) = 0.49g
• Volume = 500 ml

To find :-

• Molarity
• Normality

Solution:-

We have the formula of finding Normality amd Molarity that is

$Molarity = \dfrac{w}{GMW} \times \dfrac{1000}{V}$

w = given weight

GMW = Gram Molecular weight

V = volume

$Normality = \dfrac{w}{GEW} \times \dfrac{1}{V}$

w = given weight

GEW = Gram equivalent weight

V = volume

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So,

$Molarity = \dfrac{w}{GME} \times \dfrac{1000}{V}$

w = 0.49 g

v = 500 ml

GMW of H2SO4 = 98g [2+32+64]

Substituting the values ,

$M = \dfrac{0.49}{98} \times \dfrac{1000}{500}$

$M = \dfrac{0.49}{98} \times 2$

$M= \dfrac{0.98}{98}$

$M = 0.01$

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$Normality = \dfrac{w}{GEW} \times \dfrac{1}{V}$

w = 0.49 g

v = 500 ml

GEW = 98/2

GEW = 49 g

Substituting the values,

$= \dfrac{0.49}{49} \times \dfrac{1000}{500}$

$= \dfrac{0.49}{49} \times 2$

$= 0.01 \times 2$

$0.02$

$N = 0.02$

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