The molality of a solute in a solvent (molar mass, `20g mol^(-1))` is `0.1 mol kg^(-1)`.
What is the mole fraction of the solute?

The molality of an aqueous solution of methanol (CH_3OH) is 1.44 mol kg ""^(-1) . The mole fraction of methanol in the solution will be

What is the molality of a solution containing 200 mg of urea (molar mass = 60 g mol^(-1) ) in 40g of water ?

What is the molality of a solution containing 200 mg of urea (molar mass 60g mol^(-1)) dissolved in 40g of water?

Percent by mass of solute (molar mass = 25 g/mol) in its aqueous solution is 30. The mole fraction and molality of the solute in solution are

Percent by mass of solute (molar mass = 25 g/mol) in its aqueous solution is 30. The mole fraction and molality of the solute in solution are

The concentrations of soluitons can be expressed in number of ways , viz : mass fraction of solute (or mass percent), Molar concentration (Molarity ) and Molal concentration (molality). These terms are known as concentration terms and also they are related with each otehr i.e., knowing one concentration terms for the solution, we can find other concentration terms also. the definition of different cencentration terms are given below: Molarity : It is number of moles of solute present in one litre of the solution. Molality : It is the number of moles of solute present in one kg of the solvent. Mole fraction =("Mole of solute")/("Moles of solute" + "Moles of solvent") If molality of the solution is given as a, then mole fraction of the solute can be calculated by Mole Fraction =(a)/(a+(100)/(M_("solvent"))),=(axxM_("solvent"))/((a xx M_("solvent")+1000)0 where a=molality and M_("solvent") =Molar mass of solvent We can change : Mole fraction hArr Molality hArr Molarity What is the mole fraction of the solute?

The density of 2.0 M solution of a solute is 1.2 g mL^(-1) . If the molecular mass of the solute is 100 g mol^(-1) , then the molality of the solution is