When 2.06 g of a nonelectrolyte solute is dissolved in water to make 505 mL of solution at 26 °C, the solution exerts an osmotic pressure of 963 torr. What is the molar concentration of the solution?

The molar concentration of the solution is 0.05162 M

Explanation:

Step 1: Data given

Mass of the nonelectrolyte solute = 2.06 grams

Volume = 505 mL = 0.505 L

Temperature = 26 °C = 299 K

Osmotic pressure =963 torr

Step 2: Calculate the molar concentration

π = i*M*R*T

⇒π = the osmotic pressure = 963 torr = 1.26711 atm

⇒i = the van't Hoff factor = for a nonelectrolyte = 1

⇒M = the molar concentration = TO BE DETERMINED

⇒R = the gas constant = 0.08206 L*atm/mol*K

⇒T = the temperature = 299.15 K

M = π / (R*T)

M = 1.26711 / (0.08206*299.15)

M = 0.05162 M

The molar concentration of the solution is 0.05162 M

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