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If 1·71 G of Sugar (Molar Mass = 342) Are Dissolved in 500 Ml of an Aqueous Solution at 300 K, What Will Be Its Osmotic Pressure? - ISC (Arts) Class 12 - Chemistry (Theory)

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Question

If 1·71 g of sugar (molar mass = 342) are dissolved in 500 ml of an aqueous solution at 300 K, what will be its osmotic pressure?

Solution

Given:

mass of sugar = 1.71 g

molar mass = 342 g

volume of solution = 500 ml

temperature = 300 K

Formula used

number of moles = `"mass of sugar"/"molar mass"`

Molarity = `"number of moles of solute"/"volume of the solution in litres"`

Osmotic pressure ⇒ `pi = CRT`

Solution: 

number of moles = `1.71/342`

= 0.005

Molarity (C) = `(0.005 xx 1000)/500`

= 0.01 M

Osmotic Pressure = CRT

`= 0.01 xx 0.083 xx 300`

= 0.249 bar

  Is there an error in this question or solution?

APPEARS IN

 2014-2015 (March) (with solutions)
Question 2.1.2 | 1.00 mark
Solution If 1·71 G of Sugar (Molar Mass = 342) Are Dissolved in 500 Ml of an Aqueous Solution at 300 K, What Will Be Its Osmotic Pressure? Concept: Relative Molecular Mass of Non-volatile Substances - Osmotic Pressure and Its Application in the Determination of Relative Molecular Mass.
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