What volume of 95% sulphuric acid (density = 1.85 g cm^(-3)) and what mass of water must be taken to prepare 100 cm^3 of 15% solution of sulphuric acid (density = 1.10 g cm^(-3)) ?

What volume of 95% sulphuric acid (density = 1.85 g cm^(-3)) and what

1.	What volume of 95% sulphuric acid (density = 1.85 g cm^(-3)) and what mass of water must be taken to prepare 100 cm^3 of 15% solution of sulphuric acid (density = 1.10 g cm^(-3)) ?
Answer» Solution :Calculation of mass of `H_2SO_4` required to PREPARE `100 cm^3` of 15% solution (d = `1.10 g cm^(-3)`) : 15% solution WOULD CONTAIN 15 g of `H_2SO_4` in 100 g of solution. Density `=("Mass.)/("Volume")` `therefore` Volume of 100 g of the solution `=("Mass")/("Density") = 100/1.10 = 90.91 cm^(3)` Thus, 90.91 cm of the given solution contain 15 g of `H_2SO_4`. `therefore`Mass of `H_2SO_4` required to prepare 100 cm of the solution `=15/90.01 xx 100 = 16.5 g` Calculation of volume of 95% `H_2SO_4` (d = `1.85 g cm^(-3)`) containing 16.5 g of `H_2SO_4` : SINCE, the given sample is 95%, the mass of the sample containing 16.5 g of `H_2SO_4` `=100/95 xx 16.5 = 17.37 g` `therefore` Volume `=("Mass")/("Density") = 17.37/1.85 = 9.39 cm^(3)` `therefore` Mass of water to be taken `=110 - 17.37 = 92.63 g`