A bottle of commercial sulphuric acid (density = 1.787 g mL^(-1)) is labelled as 86 per cent by mass What is the molarity of the acid ? What volume of the acid has to be used to make 1 liotre of 0.2 M H_(2)SO_(4) ?

A bottle of commercial sulphuric acid (density = 1.787 g mL^(-1)) is l

1.	A bottle of commercial sulphuric acid (density = 1.787 g mL^(-1)) is labelled as 86 per cent by mass What is the molarity of the acid ? What volume of the acid has to be used to make 1 liotre of 0.2 M H_(2)SO_(4) ?
Answer» Solution :Step I. Calculation of molarity of the ACID solution. `"MASS of solution"=100 g, "Density of solution "=1.787"gm L"^(-1)` `"Volume of 100 g of solution"=("Mass")/("Density")=((100g))/((1.787" gm L"^(-1)))=55.9mL=0.0559 L.` `"Molarity of solution (M)"= ("Mass of" H_(2)SO_(4)//"Molar mass")/("Volume of solution in Litres")=((86g)//(98"g mol"^(-1)))/((0.0559L))` `=15.7" mol L"^(-1)=15.7 M.` Step II. `"Volume of "H_(2)SO_(4)"required".` `"Applying molarity equation," M_(1)V_(1)=M_(2)V_(2)` `(15.7 M)xxV_(1)=(0.2 M)xx(1L)` `V_(1)=((0.2M)xx(1L))/((15.7M))=0.0127xx1000=12.7 mL.`