What is the boiling point of an aqueous solution of a nonelectrolyte that has an osmotic pressure of 10.50 atm at 25°C? K_b of water is 0.52°C/m.Assume the density of the solution is the same as that of pure water. A)0.22°C B)0.429°C C)99.78°C D)100.22°C E)100.43°C

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The correct answer is B because the boiling point of an aqueous solution of a nonelectrolyte is given by the equation:Tb = Kb * mwhere Tb is the boiling point of the solution, Kb is the boiling point elevation constant of the solvent, and m is the molality of the solution.In this case, we are given that the osmotic pressure of the solution is 10.50 atm at 25°C. We can use the van't Hoff equation to calculate the molality of the solution:π = MRTwhere π is the osmotic pressure, M is the molarity of the solution, R is the ideal gas constant, and T is the temperature in Kelvin.Substituting the given values into the van't Hoff equation, we get:10.50 atm = M * 0.0821 L * atm / (mol * K) * (25 + 273) KSolving for M, we get:M = 0.500 mol/kgNow we can substitute the molality of the solution into the boiling point elevation equation:Tb = Kb * mTb = 0.52°C/m * 0.500 mol/kgTb = 0.26°CTherefore, the boiling point of the solution is 0.26°C higher than the boiling point of pure water, which is 100.00°C. So the boiling point of the solution is 100.26°C.

What Is the Boiling Point of an Aqueous Solution of a Nonelectrolyte