What volume of `HCI` solution of density `1.2g/cm^3` and containing `36.5%` by mass `HCI`, must be allowed to react wtih zinc `(Zn)` in order to liberate `4.0 g` of hydrogen ?

The molarity of 20% by mass H_(2)SO_(4) solution of density 1.28 g cm^(-3) is :

The molarity of 20% by mass H_(2)SO_(4) solution of density 1.02 g cm^(-3) is :

The density of a solution containing 7.3% by mass of HCl is 1.2 g/mL. Calculate the molarity of the solution

The density of a solution containing 7.3% by mass of HCl is 1.2 g/mL. Calculate the molarity of the solution

What volume of 95 % sulphuric acid (density 1.85 g cm^-3 ) and what mass of water must be taken to prepare 100 cm^3 of 15% solution of sulphuric acid (d = 1.1 g cm^-3) ?

The density of a solution containing 40% by mass of HCl is 1.2 g/mL. Calculate the molarity of the solution.

What volume of 95% sulphuric acid (density = 1.85 g cm^(-3) ) and what mass of water must be taken to prepare 100 cm^3 of 15% solution of sulphuric acid (density = 1.10 g cm^(-3) ) ?

100 g of HCI solution with relative density 1.117 g/ml contains 33.4 g of HCI. What volume of this HCI solution will be required to exactly neutralize 5 litre of N/10 NaOH solution?

100 g of HCI solution with relative density 1.117 g/ml contains 33.4 g of HCI. What volume of this HCI solution will be required to exactly neutralize 5 litre of N/10 NaOH solution?