The concentrated sulphuric acid that is peddled commercially is 95% `H_(2)SO_(4)` by weight. If the density of this commerical acid is `1.834 g cm^(-3)`, the molarity of this solution is

The concentrated sulphuric acid that is peddled commercially is 95% H_(2)SO_(4) by weight. If the density of this commercial acid is 1.834 g cm^(-3) , the molarity of this solution is

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

Concentrated sulphuric acid has a density of 1.9 g/mL and is 99% H_2SO_4 by weight. Calculate the molarity of H_2SO_4 in this acid.

A sample of concentrated sulphuric acid used in the laboratory is 98% by mass in aqueous solution. If the density of the solution is 1.835 g mL^-1 . Calculate the molarity of the sulphuric acid sample.

Concentrated aqueous sulphuric acid is 98% H_(2)SO_(4) by weight and has a density of 1.80 gmL^(-1) . Molarity of solution

Calculate molality of 1 litre solution of 95% H_(2) SO_(4) by volume. The density of solution is 1.84 g mL^(-1) .

Commercially available sample of sulphuric acid is 15% H_2SO_4 by weight (density=1.10g mL^-1 ) . Calculate the molarity of the solution.

Find the molarity and molality of a 14% solution of H_(2) SO_(4) by weight. The density of the solution is 1.10 g/cc and the molecular mass of sulphuric acid is 98