(a) Define the following terms :
(i) Ideal solution (ii) Azeotrope (iii) Osmotic pressure
(b) A solution of glucose `(C_(6)H_(12)O_(6))` in water is labelled as 10% by weight. What would be the molality of the solution? (Molar mass of glucose= 180 g `mol^(-1)`)

Define the following terms, (a) Ideal solution. (b) Azeotrope. (c) Osmotic pressure. (ii) A solution of glucose (C_(6)H_(12)O_(6)) in water is labelled as 10% by weight what would be the molality of the solution ? (Molar mass of glucose=180 g mol^(-1) )

Define the following terms: (i) Ideal solution (ii) Molarity (M)

What would be the molality of 20% (mass/mass) aqueous solution of Kl? (molar mass of Kl = 166 g mol^(-1) )

A solution of glucose ("molar mass"= 180g mol^(-1)) in water is labelled as 10% (by mass). What would be the molarity and molality of the solution? Given that the density of the solution is 1.2g mL^(-1) .

What would be the molality of 10% (mass/mass) aqueous solution of KI ? (molar mass of KI = 166 g mol^(-1) )

What would be the molality of 20% (mass/mass) aqueous solution of KI ? (molar mass of KI = 166 g mol^(-1) )

What will be the molality of a solution of glucose in water which is 10% w //W ?

If the concentration of glucose (C_(6)H_(12)O_(6)) in blood is 0.9 g L^(-1) , what will be the molarity of glucose in blood?

If the concentration of glucose (C_(6)H_(12)O_(6)) in blood is 0.9 g L^(-1) , what will be the molarity of glucose in blood?

(a) What type of deviation is shown by a mixture of ethanol and acetone? Give reason (b) A solution of glucose (molar mass =180 g mol^(-1)) in water is labelled as 10% (by mass) what would be the molality and molarity of the solution ? (Density of solution =1.2 gL^(-1))