Determine the concentration of an aqueous solution that has an osmotic pressure of 3.9 atm at 37°C if the solute is sodium chloride. Assume no ion pairing.

Question

Ingrid Pearson

Chemistry

12 October, 05:24

Determine the concentration of an aqueous solution that has an osmotic pressure of 3.9 atm at 37°C if the solute is sodium chloride. Assume no ion pairing.

+1

Answers (1)

Know the Answer?

Brayan Bernard · Answer 1

Concentration for the solution is 0.153 mol/L

Explanation:

Formula for the osmotic pressure is π = M. R. T. i

where M is molarity (concentration), R the universal constant for gases and T is Absolute T° (T°C + 273)

π = Osmotic pressure.

Let's replace the data given:

3.9 atm = M. 0.082L. atm/mol. K. 310K

3.9 atm / 0.082 mol. K/L. atm. 310K = 0.153 mol/L (M)

i = Van't Hoff factor (ions from the solute dissolved in solution)

In this case, we assumed no ion pairing, so i = 1