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What volume of 95% sulphuric acid (density = 1.85 g/mL) and what mass of water must be taken to prepare 100 mL of 15% solution of sulphuric acid (density = 1.10 g/mL) ?
Asked by abhinavsaini123 | 06 Jul, 2015, 09:16: AM
To find:
Volume of 95% sulphuric acid (density = 1.85 g/mL)
Mass of water to prepare 100 mL of 15% solution of sulphuric acid (density = 1.10 g/mL)

Solution:

Volume of the solution = 100 cm2

Density of the solution = 1.10 g/cm3

Therefore, Mass of 100 cm3 of solution = 100 x 1.10 g =110 g

The given solutions is 15%. Therefore, 100 g of solution contains 15 g of H2SO4

Then, mass H2SO4 in 110 g (100 cm3 ) of solution =

Mass of water in 110 g (100cm3 ) of solution = (110 - 16.5) g = 93.5 g

To obtain 100 cm3 of 15 % solution acid, we require the given information.

Mass of water = 93.5 g

Mass of H2SO4 (100% pure) = 16.5 g

Since, the given sulphuric acid is 95% pure, hence,

Mass of H2SO4 (95%) will be required =

Answered by Hanisha Vyas | 06 Jul, 2015, 12:46: PM

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