If you make a solution by dissolving 1.0 mol of fecl3 into 1.0 kg of water, how would the osmotic pressure of this solution compare with the osmotic pressure of a solution that is made from 1.0 mol of glucose in 1.0 kg of water? one-half as large the same twice as large four times as large

Calculating the osmotic pressure of solution:

Osmotic pressure, π = iMRT

FeCl3 gives 1 ion and 3 ions.

i = 1 + 3 = 4

Calculating molarity:

Mass of solvent = 1.0 kg or 1000 g

Mass of =

Total solution mass = 1000 g + 162.20 g = 1162.20 g

Volume of solution =

                                =

Molarity =

Osmotic pressure = 4 * 0.86 M (0.08206 L.atm/(mol.K)(298K)

                              = 84. atm

(We assume T is standard temperature and density of both solutions = 1 g/mL)

Calculating the osmotic pressure of glucose solution:

Osmotic pressure, π = iMRT

i = 1 (as glucose is non electrolyte)

Calculating molarity:

Mass of solvent = 1.0 kg or 1000 g

Mass of glucose =

Total solution mass = 1000 g + 180.16 g = 1180.16. g

Volume of solution =

                                =

Molarity =

Osmotic pressure = 1 * 0.85 M (0.08206 L.atm/(mol.K)(298K)

                              = 21. atm

So when we compare, the osmotic pressures of 1.0 mol of FeCl3 dissolved into 1.0 kg of water is 4 times the osmotic pressure of  1.0 mol of glucose in 1.0 kg of water

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