The density of `2% ` (W//W)` aqueous KI solution is 1.202 `g mL^(-1)` . What is the approximate molaility ? Molar mass of Ki =166 )

The density of 20% (w/w) aqueous NaOH solution is 1.20 g. mL^(-1) . What is the mole fraction of water ? (molar mass of NaOH = 40g. "mol"^(-1) )

The density of 4% (w/v) NaOH solution is 1.02 g/ml. What is the molality of the solution ?

%(w/v) of aqueous KOH solution is 1.4. What is the molarity of solution? (Molar mass of KOH= 56)

%(w/v) of aqueous KOH solution is 1.4 What is the molarity of solution? (Molar mass of KOH= 56 )

An aqueous solution of sodium chloride is marked 10%(w//w) on the bottle. The density of the solution is 1.071 gmL^(-1) . What is the molity and molarity? Also, what is the mole fraction of each components in the solution?

Calculate a) molality b) molarity and c) mole fraction of KI if the density of 20% (mass / mass) aqueous KI is 1.202" g mL"^(-1) . As density and % by mass is given, so find the mass of solute and solvent (as x % solution contains x g solute in (100 - x) g solvent). Find volume of the solution, by using,, Volume =("Mass")/("Density") Recall the formulae of molality, molarity and mole fraction, to calculate them. Molality =("Mass of solute/ molar mass of solute")/("Mass of solventin kg")

Calculate mole fraction of KI if density of 20% (mass/mass) aqueous solution of KI is 1.202 gmL^-1 ?

Calculate the molarity of Kl if the density of 20% (mass/mass) aqueous Kl is 1.202 " g mL"^(-1)

A 30% (W/W) aqueous solution has density 2gm/ml and molarity 2M, then molar mass of solute is: