A compound `H_2X` with molar weight of 80 g is dissolved in a solvent having density of 0.4 g `ml^-1`. Assuming no change in volume upon dissolution, the molality of a 3.2 molar solution is

A compound H_2X with molar weight of 80 g is dissolved in a solvent having density of 0.4 g ml^(-1) Assuming no change in volume upon sdissolution, the molality of a 3.2 molar solution is

The pH of a solution of H_2SO_4 is 1. Assuming complete ionisation, find the molarity of H_2SO_4 solution

4.5g of urea (molar mass = 60g "mol"^(-1) ) are dissolved in water and solution is made to 100 ml in a volumetric flask. Calculate the molarity of solution.

An aqueous solution of NaOH having density 1.1. kg /dm^3 contains 0.02 mole fraction of NaOH. The molality and molarity of NaOH solution respectively are

The molarity of a NaOH solution by dissolving 4g of it in 250 ml water is

The normality off 10% H_(2)SO_(4) solution having density 1.1g/cc is-

35 drops of a liquid having density 1.2 g/mL, weigh 2.4 g. assuming molecular weight of liquid 70, select the correct statements

The density of a solution prepared by dissolving 120g of urea (mol. Mass=60u) in 1000g of water is 1.15 g*mL^(-1) . The molarity of this solution is-

29.2% (wiW) HCI stock solution has density of 1.25 g mL^-1 . The molecular weight of HCl is 36.5 g mol^-1 . The volume (mL) of stock solution required to prepare a 200 mL solution 0.4 M HCI is

0.900g of a solute was dissolved in 100 ml of benzene at 25^(@)C when its density is 0.879 g/ml. This solution boiled 0.250^(@)C higher than the boiling point of benzene. Molal elevation constant for benzene is "2.52 K.Kg.mol"^(-1) . Calculate the molecular weight of the solute.