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Solution by mass and has a density of $1.80 g m L − 1$ . The volume of acid required to make $1 L$ . The volume of acid required to make of $0.1 M H 2 S O 4$ of solution $98 % H 2 S O 4$ solution is [[1]] mL.

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Detailed Solution

Concept: The required volume is 5.55 mL. The molarity of a solution is the number of moles of solute per litre of the solution by mass

98 % H 2 S O 4

giving the idea that it contains 98 g acid in 100 g solution.
One molar solution means one mole of acid per litre solution. The molar mass of

H 2 S O 4

is 98 g. So the given solution is 1 molar solution with a density of

1.80 g m L − 1

. We can calculate the amount of acid needed to make

0.1 M

the solution as follows-

1 M = 98 g 0.1 M = ? 1 × 98 0.1 = 9.8 g

Now the question is to find the volume of the acid. To convert the calculated amount in mass to volume, we can use density.

D e n s i t y = M a s s V o l u m e V o l u m e = M a s s D e n s i t y = 9.8 1.80 = 5.5 m L

The volume of the acid to make

0.1 M

the solution is

5.5 m L

.
Hence, the correct answer is 5.55 mL.

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