The molarity (in mol/liter) of a `13%` solution (by weight) of sulphuric acid with a density of `1.02g//mL` is (Note Report your answer in the required format by relevant rounding up.)

What is the molarityk and molality of a 13% solution (by weight) of sulphric acid with a density of 1.02 mL^(-1) ? To what volume should 100 mL of this acid be diluted in order to preapre a 1.5 N solution?

The molarity of 20% (W/W) solution of sulphuric acid is 2.55 M. The density of the solution is :

The density of a solution containing 13% by mass of sulphuric acid is 1.09g//mL . Calculate the molarity and normality of the solution

The density of a solution containing 13% by mass of sulphuric acid is 1.09 g..mL . Calculate the molarity and normality of the solution.

Density of a solution containing 13% by mass of sulphuric acid is 0.98 g/mL. Then molarity of solution will be

Concentrated sulphuric acid has density of 1.9 g/mL and 99% H_(2)SO_(4) by mass. Calculate the molarity of the acid.