Solutions Test ...

90 gm glucose and 120 gm urea dissolved in 1.46 kg aqueous solution, then what will be the boiling point of the solution at 1 bar pressure ? (Kb = 0.512^o C -kg – mole^-1, molecular weight of glucose and urea are 180 and 60 gm/mole respectively)

pH of 0.2M dibasic acid H₂A is 1.699; then, what will be its osmotic pressure at T K temperature ?

Boiling point of an aqueous soultion of 0.4m AlCl₃ is 100.7_oC; then what would be the pressure of ionization of AlCl₃ ? Kb – 0.512^o C - kg - mole^-1.

The vapour pressure of homogenous mixture of 10 mole of liquid X and 30 mole of liquid Y at constant temperature is 550 mm. In this solution, 10 mole of liquid Y increases, hence, increase in vapour pressure is 10 mm. Then, find the vapor pressure of pure liquid X and Y at that temperature.

What amount of urea dissolved in 1 kg water at constant temperature, so that vapour pressure of the solution reduced by 2% ? ( M.W of urea = 60 gm/mole)

What would be tne volume of 15% w/v and 5% w/v NaOH solution required to prepare 1 litre aqueous solution of 2M NaOH ? (M.w of Naoh = 40 gram/mole)

At constant temperature, vapour pressure of an aqueous solution of 1.5 kg glucose decreases to 0.98% in comparision with vapour pressure of pure water then, what quantity of glucose in gram dissolved in the solution ? (Molecular weight of glucose = 180 gm/mole)

At constant pressure, 0.5 m NaCl aqueous solution is diluted by adding water in it. Which of the following statement is correct in this reference ?

Boiling point of an aqueous solution of 0.5 m ionic solid substance is 100.5^oC; then state the value of i ? (Kb = 0.512^oC -kg – mole^-1)

Aqueous solution of substance boils at 100.5^oC at 1 bar pressure; then at what temperature it freezes ? (K_b = 0.512^oC -k_g - mole^-1, K_f = 1.86^oC - k_g – mole^-1)