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.

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

the answer for sodium is 0.186

the answer for rubidium is 0.251

b. is the answer hoped i