Share

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)

ConceptRelative Molecular Mass of Non-volatile Substances Osmotic Pressure and Its Application in the Determination of Relative Molecular Mass

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.
S