Question

What is the osmotic pressure of a 0.050 m solution of alcl3 in water that is at 0.00°c? consider alcl3 to be a strong electrolyte?

Answer 1

Answer: Osmotic pressure of the given solution is 4.48 atm.

Step-by-step explanation: Osmotic pressure is defined as the number of moles of solute which are present in a solution.

Mathematically,

`\pi = icRT` ....(1)

where i = Van't Hoff factor

c = concentration of the solution

R = Universal gas constant =
`0.0821\text{ atm L }mol^(-1)K^(-1)`

T = temperature of the solution

Value of 'i' is 1 for non-electrolytes. But, here
`AlCl_3` is an electrolyte, so the value of Van't Hoff factor will be the number of moles of particles of solute we get when 1 mole of solute is dissolved in a solution.

So, when 1 mole of
`AlCl_3` dissociates in aqueous state to produce 1 mole of
`Al^(3+)` ion and 3 moles of
`Cl^-` ion.

`AlCl_3(aq.)\rightarrow Al^(3+)(aq.)+3Cl^-(aq.)`

For
`AlCl_3`,

i = 4

c = 0.050 mol/L

T = (273 + 0)K = 273 K

Putting the values in equation 1, we get

`\pi =4*0.050mol/L*0.0821\text{ atm L }mol^(-1)K^(-1)* 273K`

`\pi =4.48atm`