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Raoult's Law

The empirical...

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The empirical formula of a non- { electrolyte/non-associating solute is CH_2O . { A solution containing 3g of the solute in 1L water exerts the same osmotic pressure as { that of 0.05M glucose solution. The molecular formula of the compound is

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Q. The empirical formula of a non-electrolyte is

C H_{2} O

. A solution containing 6g of the compound exerts the same osmotic pressure as that of 0.05 M glucose solution at the same temperature. The molecular formula of the compound is:

6 %

glucose solution and

2 %

solution of X show same osmotic pressure. Assuming X to be a non-electrolyte, the molecular weight of X is

Q. A solution containing

1.8 g

of a non-electrolyte (empirical formula

C H_{2} O

40 g

of water is observed to freeze at

- {0.465}^{\circ} C

. The molecular formula of the compound is:
(

K_{f}

= 1.86 {kg K mol}^{- 1})

Q. Solute A is a ternary electrolyte and solute B is a non-electrolyte. If 0.1 M solution of solute B produces an osmotic pressure of 2P, then 0.05 M solution of A at the same temperature will produce an osmotic pressure equal to:

Q. An electrolyte

A

3

B

is a non- electrolyte. If

0.1 M

B

produces an osmotic pressure

P

0.05 M

A

will produce an osmotic pressure, assuming that the electrolyte is completely ionised:

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