When 2.46g of a nonelectrolyte solute is dissolved in water to make 115 ml of so

Question

When 2.46g of a nonelectrolyte solute is dissolved in water to make 115 ml of solution at 25 degrees C, the solution exerts an osmotic pressure of 959 torr.
A) what is the molar concentration of the solution?
B)how many moles of solute are in the solution?
C)what is the molar mass of the solute? When 2.46g of a nonelectrolyte solute is dissolved in water to make 115 ml of solution at 25 degrees C, the solution exerts an osmotic pressure of 959 torr.
A) what is the molar concentration of the solution?
B)how many moles of solute are in the solution?
C)what is the molar mass of the solute?
A) what is the molar concentration of the solution?
B)how many moles of solute are in the solution?
C)what is the molar mass of the solute?

Explanation / Answer

A)
Osmoticpressure = CRT

959 torr = 1.26184211 atm

1.26184 = C*0.0821*298

C = concentration = 0.051574 M

B) No of moles of solute = 0.051574*0.115 = 0.00593101 mol

c) Molarmass of solute = 2.46/0.00593101 = 414.769 g/mol

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