Asolution is prepared by dissolving 4.78 g of an unknown nonelectrolyte in enough water to make 375 ml of solution. the osmotic pressure of the solution is 1.33 atm at 27c. what is the molar mass of the solute?

Answers

answer carbon and three oxygen atoms;

The answer options is d

The molar mass of the solute is 236.0 g/mol

Explanation:

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

\pi=iMRT

where,

\pi = osmotic pressure of the solution = 1.33 atm

i = Van't hoff factor = 1 (for non-electrolytes)

M = molarity of solute = ?

R = Gas constant = 0.0821\text{ L atm }mol^{-1}K^{-1}

T = temperature of the solution = 27^oC=[273+27]K=300K

Putting values in above equation, we get:

1.33atm=1\times M\times 0.0821\text{ L.atm }mol^{-1}K^{-1}\times 300K\\\\M=\frac{1.33}{1\times 0.0821\times 300}=0.0540M

To calculate the molecular mass of solute, we use the equation used to calculate the molarity of solution:

\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}

We are given:

Molarity of solution = 0.0540 M

Given mass of solute = 4.78 g

Volume of solution = 375 mL

Putting values in above equation, we get:

0.0540M=\frac{4.78\times 1000}{\text{Molar mass of solute}\times 375}\\\\\text{Molar mass of solute}=\frac{4.78\times 1000}{0.0540\times 375}=236.0g/mol

Hence, the molar mass of the solute is 236.0 g/mol



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