# When 3.25 g of a nonelectrolyte solute is dissolved in water to make 165 mL of solution at 24 °C, the solution exerts an osmotic pressure of 879 torr.What is the molar concentration of the solution? MHow many moles of solute are in the solution? molWhat is the molar mass of the solute? g/mol

Question

When 3.25 g of a nonelectrolyte solute is dissolved in water to make 165 mL of solution at 24 °C, the solution exerts an osmotic pressure of 879 torr.
What is the molar concentration of the solution? M
How many moles of solute are in the solution? mol
What is the molar mass of the solute? g/mol

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Step 1

Osmotic pressure (p) of a solution is a colligative property, meaning it depends upon the concentration of solute (M) in solution.

Step 2

Give here, a solution made with a non-electrolyte solute in water exerts an osmotic pressure of 879 torr.

convert osmotic pressure from torr to atm

conversion factor, 1 atm = 760 torr

So,

879 torr = 879 torr x 1 atm/760 torr = 1.16 atm

Using formula,

p = iMRT

with,

osmotic pressure (p) = 1.16 atm

i (Van't hoff factor) = 1 (nonelectrolyte)

R = 0.08206 L.atm/K.mol

M = concentration of solution = ?

T = 24 + 273 = 297 K

So,

1.16 = 1 x M x 0.08206 x 297

M = 0.05 M

(a) So the concentration of solution = 0.05 M

Step 3

(b) Calculate moles of solute in solution

Given,

Volume of water (solvent) = 165 ml = 0.165 L

[1 L = 1000 ml]

Molarity of solution = 0.05 M

Using,

moles = molarity x volume (M)

&nb...

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