Question

Calculate the molarity of a solution of H2SO4 which contains 5.5 gm of acid in 300 ml of solution?

Answer 1

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Answer 2

The molarity of a solution $H_{2}SO_{4}$ that contains 5.5 gm of acid in 300 ml of solution is 0.186 M.

Given: the amount of acid: 5.5gm

           the volume of solution: 300ml

to find:  the molarity of a solution of $H_{2}SO_{4}$

Solution:

Molarity is the total number of solutes dissolved in 1 litre ie 1000ml of solution.

M = Total number of moles of solute ÷ volume of solution in litres

molecular weight of $H_{2}SO_{4}$ = 98g/mol

total number of moles of solute = amount of acid÷ molecular weight of acid

total number of moles of solute = 5.5 g ÷ 98 g/mol

total number of moles of solute = 0.056 moles

the volume of solution in liters= 300 ml ÷ 1000 ml= 0.3 l

Molarity of solution= 0.056 moles ÷ 0.3 l = 0.186 M

Hence the molarity of a solution of H2SO4 which contains 5.5 gm of acid in 300 ml of solution is 0.186 M.

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