A bottle of commercial sulphuric acid `(d = 1.787 g mL^(-1))` is 86% by weight.
a. What is molarity of the acid?
b. What volume of the acid has to be used to make `1 L` of `0.2 M H_(2) SO_(4)`?
c. What is the molality of the acid?

Answer

12.65

Explanation

Molarity `=("Mass of solute /M. wt. of solute")/("Mass of solution/density of solution") xx 1000`
`M = (86//98)/(100//1.787) xx 1000`
`=0.8775/55.5 xx 1000 = 15.81` M
Now, `(M_(1)V_(1)) = (M_(2)V_(2))`
`therefore 15.81 xx V_(1) =0.2 xx 1000`
`therefore` Amount of acid to be used to make 1 L of 0.2 M.
`H_(2)SO_(4) = 12.65`