The normality of 4.9% (w/w) H2SO4 Solution having density 1.02 g / ml is ?

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Solution

4.9 % acid by mass means 4.9g acid in 100 g solution.
Density = 1.02 g/mL
Volume of solution = Mass /density
= 100/1.02
= 98.03 ml
Molar mass sulphuric acid H₂So₄ = 21 + 32 + 416 = 98g/mol
Number of moles of sulphuric acid = mass / molar mass
=4.9 / 98
=0.05
Molarity = number of moles / volume of solution in litres
= 0.05 / 0.9803
= 0.051 M
Normality = Molarity * Basicity
= 0.051*2 =0.102 N
Hence, the normality of 4.9% of H₂So₄ of density 1.02g/ml is 0.102N

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