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For a dilute solution containing 2.5 g of a non-volatile, non-electrolyte solute in 100 g of water, the elevation in boiling point at 1 atm pressure is `2^@C`. Assuming concentration of solute is much lower than the concentration of solvent, the vapour pressure (mm of Hg) of the solution is `(K_b = 0.76 K kg mol^(-1))`

A

726

B

740

C

736

D

718

Text Solution

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The correct Answer is:
A
726
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For a dilute solution containing 2.5g of a non-volatile non-electrolyte solute in 100g of water, the elevation in boiling point at 1 atm pressure is 2^(@)"C" . Assuming concentration of solute is much lower than the concentration of solvent, the vapour pressure (mm of Hg) of the solution is (take K_(b) =0.76 K kg "mol"^(-1) )

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For a dilute solution containing 2.5 g of a non-voltile and non-electrolyte solute in 100 g of water, the elevation in boiling at 1 atm pressure is 2^(@)C . Assuming that the concentration of solute is mich less lower that the concentration of the solvent, what is the capour pressure (mm of Hg) of the solution? Given K_(b)=0.76 K kg mol^(-1) )

A solution containing 12.5 g of non - electrolyte substance in 175 g of water gave boiling point elevation of 0.70 K. Calculate the molar mass of the substance. Elevation constant (K_(b)) for water "0.52 K kg mol"^(-1) ?

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