Solutions

We have three aqueous solutions of NaCl labelled as 'A', 'B' and 'C' with concentration 0.1 M, 0.01 M and 0.001 M, respectively. The value of van 't Hoff factor (i) for these solutions will be in the order :

1. iA < iC < iB
2. iA < iB < iC
3. iA > iB > iC
4. iA = iB = iC

Mass of ethylene glycol (antifreeze) to be added to 18.6 kg of water to protect the freezing point at -24 is kg (Molar mass in g mol-1 for ethylene glycol 62, Kf of water = 1.86 K kg mol-1)

Identify the mixture that shows positive deviations from Raoult's Law

1. (CH3)2CO + CS2
2. (CH3)2CO + C6H5NH2
3. CHCl3 + C6H6
4. CHCl3 + (CH3)2CO

What happens to freezing point of benzene when small quantity of naphthalene is added to benzene?

1. Increases
2. Decreases
3. Remains unchanged
4. First decreases and then increases

The solution from the following with highest depression in freezing point/lowest freezing point is

1. 180 g of acetic acid dissolved in benzene
2. 180 g of acetic acid dissolved in water
3. 180 g of benzoic acid dissolved in benzene
4. 180 g of glucose dissolved in water

If a substance 'A' dissolves in solution of a mixture of 'B' and 'C' with their respective number of moles as nA, nB and nC. Mole fraction of C in the solution is

1. nCnA nB nC
2. nBnA+nB
3. nCnA+nB+nC
4. nCnA-nB-nC

The osmotic pressure of a dilute solution is 7 105 Pa at 273 K. Osmotic pressure of the same solution at 283 K is 104 Nm-2.

Molality of 0.8 M H2SO4 solution (density 1.06 g cm-3) is 10-3 m.

A solution of two miscible liquids showing negative deviation from Raoult's law will have :

1. increased vapour pressure, increased boiling point
2. increased vapour pressure, decreased boiling point
3. decreased vapour pressure, decreased boiling point
4. decreased vapour pressure, increased boiling point

The quantity which changes with temperature is :

1. Molality
2. Molarity
3. Mole fraction
4. Mass percentage