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

The volume of a body having density 1 g cm^(-3) and mass 100 g is _____ cm^(3) .

The volume of a body having density 1 g cm^(-3) and mass 100 g is _____ cm^(3) .

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

100 ml of 5 M NaOH solution (density 1.2 g/ml) added to 200 mL of another NaOH solution which has a density of 1.5 g/ml and contains 20 mass percent of NaOH. What will be the volume of the gas (at STP) in litres liberated when aluminium reacts with this (final) solution? [Give answer excluding decimal places] The reaction is Al+NaOH+H_(2)OrarrNaAlO_(2)+H_(2) (At. wt. Na=23, 0=16, H=1)

How many milliliter of conc. HCI of specific gravity 1.19 and which contains 37% by mass HCI will be required to prepare 2 litre of decinormal 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?