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The freezing point order of the solution of glucose is
An experimenter tries to determine the molecular weight of glucose by observing the depression in freezing point. He carries out his experiment in duplicate. In one he uses pure water as the solvent and in the other experiment, by mistake he uses a 0.1N aqueous NaCl as the solvent. It is expected that he will report
How many moles of glucose should be added to 1000 g of water so that the freezing point is depressed by 0.93 K ? Assume ${{K}_{f}}$ for water to be 1.86 K Kg$mo{{l}^{-1}}$
Two solutions of $KN{{O}_{3}}$ and $C{{H}_{3}}COOH$ are prepared separately. Molarity of both is $0.1M$ and osmotic pressures are ${{P}_{1}}$ and ${{P}_{2}}$ respectively. The correct relationship between the osmotic pressures is
The osmotic pressure of 1 m solution at 27°C is
The concentration in gms per litre of a solution of cane sugar ($M=342$) which is isotonic with a solution containing $6\ gms$ of urea ($M=60$) per litre is
The value of osmotic pressure of a $0.2M$ aqueous solution at $293K$ is
The relationship between osmotic pressrue at $273K$ when $10g$ glucose $({{P}_{1}})$, $10g$ urea $({{P}_{2}})$ and $10g$ sucrose $({{P}_{3}})$ are dissolved in $250ml$ of water is
The osmotic pressure of 0.4% urea solution is 1.66 atm and that of a solution of sugar of 3.42% is 2.46 atm. when both the solution are mixed then the osmotic pressure of the resultant solution will be
A solution of urea contain 8.6 gm/litre (mol. wt. 60.0). It is isotonic with a 5% solution of a non-volatile solute. The molecular weight of the solute will be

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