A sample of commercial sulphuric acid is `98% H_(2) SO_(4)` by mass. Calculate the mole fractions of `H_(2) SO_(4)` and `H_(2) O`.

Calculate the equivalent mass of H_(2) SO_(4) .

Molarity: A sample of commercial sulphuric acid is 98% H_(2) SO_(4) by mass and its specfic gravity is 1.84 . Caculate the molartiy of this sulburic acid solution. Strategy: The density of a solution (grams per milliliter) is numercially equal to its specific gravity. Thus, the density of the solution is 98% H_(2) SO_(4) by mass. Thus, every 100g of soultuon contains 98g of pure H_(2) SO_(4) . From the mass of H_(2) SO_(4) . we calculate its moles and from the density , we calculate its volume. Finally, we calculate molartity using its definition.

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

Calculate the molar mass of sulphuric acid (H_(2)SO_(4)) .

A mixture is prepared by mixing 10 gm H_(2)SO_(4) and 40 gm SO_(3) calculate mole fraction of H_(2)SO_(4)

The molecular mass of H_(2)SO_(4) is 98 amu . Calculate the number of moles of each element in 294 g of H_(2)SO_(4) .

What is the density of 3.60 M sulphuric acid, which is 29% H_(2)SO_(4) by mass?