total mol = mol of B + mol of A
xb = mol of B / total mol
xb = mol of B / (mol of A + mol of B)
xa = mol of A / (mol of A + mol of B)
then...
if we assume Mb = mol of B / kg of solvent
and assume solvent = A
then
Mb = mol of B / kg solvent
kg of solvent = kg of A = mass of A = mol of A * MW of A
so
Mb = mol of B / (mol of A * MW of A)
solve for mol of B
mol of B = Mb* ((mol of A * MW of A)) =
substitute
xb = mol of B / (mol of A + mol of B)
xb =Mb* ((mol of A * MW of A)) / (mol of A + Mb* ((mol of A * MW of A))
for A:
xa = mol of A / (mol of A + Mb* ((mol of A * MW of A))
For a binary solution, find expressions for the mole fractions x_B and x_A as functions of...
For a binary solution, find expressions for the mole fractions xB and xA as functions of the solute molality mB.
In an azeotropic solution, the liquid and vapor phases have equal mole fractions of solute at equilibrium. Find the numerical value of the Henrt's Law coefficient that is azeotropic at its standard boiling point. Include units.
How do you find the mass percent, mole fraction, and the
molality for these two problems?
P1. (Sec. 11.1) A solution is prepared by dissolving 113 grams of acetone (C3H6O) in 662 grams of water. With this information, calculate the solution's mass percent % of the solute, mole fraction of the solute, and the solutions molality. a) b) c) d) e) Mass Percent: 88.7%; Mole Fraction (Solute): 0.9068; & Molality: 5.70 mol/kg Mass Percent: 11.3%; Mole Fraction (Solute): 0.0932; &...
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At 100 ?C the vapor pressures of hexane and octane are 1836 and 354 torr, respectively. A certain liquid mixture of these two compounds has a vapor pressure of 666torr at 100 ?C. Find the mole fractions in the liquid mixture and in the vapor phase. Assume an ideal solution.
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Calculate the molality of an aqueous solution of iron (II) nitrate with a solute mole fraction of 0.062 and a density, ρ = 1.045 g/mL. Report your answer to THREE significant figures
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