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Sagot :
0.0105 mol of non-electrolyte solute, with 297.14 g/mol molar mass, is dissolved in water to make a 0.0488 M solution.
Given:
- mass of solute (m) = 3.12 g
- volume of solution (V) = 215 mL
- Temperature (T) = 27 deg C or 300 K
- Gas-constant (R) = 0.08206 L-atm/mol-K
Osmotic pressure is expressed mathematically as π=M*R*T. The concentration of the solution "M" should be expressed in molarity, mol/L. Through the use of the formula, let us solve for the concentration of the solution. The osmotic pressure must be converted to atm.
Conversion factor: 1 atm has 760 torr.
913 torr * (1 atm/760 torr) = 1.20131 atm
Ï€ = 1.20131 atm = M*(0.08206 L-atm/mol-K)*(300 K)
M = 0.0488 M
From the molar concentration of the solution, we can solve for the number of moles of the solute.
M = mol solute / volume solution
mol solute = M * volume solution
mol solute = 0.0488 M * (215 mL) * (1 L/1000 mL)
mol solute = 0.0105 mol
Then, we can solve for the molar mass of the solute.
molar mass solute = mass solute / mol solute
molar mass solute = 3.12 g / 0.0105 mol
molar mass solute = 297.14 g/mol
To learn more about osmotic pressure, please refer to https://brainly.com/question/8195553.
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