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Chemistry
Properties of solutions
Freezing Point Depression
freezing point of pure solvent remains constant whereas the freezing point of a solution continues to decrease with time
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sounds reasonable.
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Explain why the freezing point of a pure solvent remains constant whereas
the freezing point of a solution continues to decrease
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This question makes no sense to me.
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The equation for lowering the freezing point of a solvent is given in your manual. Given that the freezing point for the pure
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Yes, delta T is 0.69. Then new freezing point is 79.4-0.69 = ? If your prof watches significant
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you are conducting a freezing-point determination in the laboratory by using an aqueous solution of KNO3. The observed freezing
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A freezing point depression experiment was conducted using cyclohexane as the solvent. The freezing point of pure cyclohexane is
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Explain why the freezing point of a pure solvent is constant, whereas the freezing point of a solution decreases with steady
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As the solution is cooled, at some point lower than the normal freezing point of the solvent, a few
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Analysis of a compound gave 39.50% C, 2.20% H, and 58.30% Cl. When 0.855 g of this solid was dissolved in 7.50 g of napthalene,
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Nah bi
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When 0.855 g of this solid was dissolved in 7.50 g of napthalene, the solution had a freezing point of 78.0° C. The pure
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delta T = Kf*molality Solve for molality molality = moles/kg solvent Solve for moles. moles =
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A solution is prepared by dissolving 5.00 g of glycerin (C3H8O3) in 201 g of ethanol (C2H5OH). The freezing point of the
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delta T = i*Kf*molality i = 1 Kf = 1.99 molality = moles glycerin/kg solvent mols glycerin = 5/molar
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The freezing point of pure cyclohexane is 6.60°C and the freezing point depression constant is 20.00°C/m. The freezing point
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Indicate your <I>specific</I> subject in the "School Subject" box, so those with expertise in the
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The freezing point of pure cyclohexane is 6.60°C and the freezing point depression constant is 20.00°C/m. The freezing point
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