Place the following solutions in order of increasing osmotic pressure.

Asked by maham237 @ 25/12/2020 in Chemistry viewed by 321 People

Place the following solutions in order of increasing osmotic pressure. I. 0.15 M C2H6O2. II. 0.15 M MgCl2, III. 0.15 M NaCl, A. III < I < II B. II < III < I C. I < II < III D. I < III < II the answer is D but how do you know?

Answered by maham237 @ 25/12/2020

Answer:

D. I < III < II

Explanation:

The osmotic pressure (π) is given by the relation:

π = iMRT.

where, π is the osmotic pressure.

i is van 't Hoff factor.

M is the molarity of the solution.

R is the general gas constant.

T is the temperature.

M, R and T are constant for all solutions.

So, the osmotic pressure depends on the van 't Hoff factor.

The van 't Hoff factor is the ratio between the actual concentration of particles produced when the substance is dissolved and the concentration of a substance as calculated from its mass.

For most non-electrolytes dissolved in water, the van 't Hoff factor is essentially 1.

For most ionic compounds dissolved in water, the van 't Hoff factor is equal to the number of discrete ions in a formula unit of the substance.

For C₂H₆O₂ (non-electrolyte solute): i = 1.

For MgCl₂: i = 3.

It dissociates to give (Mg²⁺ + 2Cl⁻).

For NaCl: i = 2.

It dissociates to give (Na⁺ + Cl⁻).

So, the solute that has the highest osmotic pressure is II. 0.15 M MgCl₂, then III. 0.15 M NaCl, then I. 0.15 M C₂H₆O₂.

So, the answer is:

D. I < III < II.

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