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SP. 10 Calculate the freezing point of a solution containing 4.27g of table sugar (C₁2H₂2011) in 50 g of water (H₂O).

SP. 10 Calculate the freezing point of a solution containing 4.27g of table sugar (C₁2H₂2011) in 50 g of water (H₂O).

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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3A. Freezing Point Depression The freezing point of a solution is less than the freezing point of the pure solvent. This means that a solution must be cooled to a lower temperature than the pure solvent in order for freezing to occur. The freezing point of the solvent in a solution changes as the concentration of the solute in the solution changes (but it does not depend on the identity of either the solvent or the solute(s) particles (kind, size or charge) in the solution). The freezing point of the solvent in a solution will be less than the freezing point of the pure solvent whether the solution contains a non-volatile solute or a volatile solute. However, for simplicity, only non-volatile solutes will be considered here. SP. 10 Freezing Point total (Tb) = Freezing Point solvent (Tisolv) - AT, AT, = K,m where: AT+ = freezing point depression K+ = freezing point depression constant m = molality of solute constants for some common solvents: Solvent Water Benzene Chloroform Normal Freezing Point, °C 0.0°C 5.5°C -63.5°C Fp depression const., °C/mol 1.86 °C/mol 5.12 °C/mol 4.68 °C/mol Calculate the freezing point of a solution containing 4.27g of table sugar (C₁2H₂2011) in 50 g of water (H₂O).
Transcribed Image Text:3A. Freezing Point Depression The freezing point of a solution is less than the freezing point of the pure solvent. This means that a solution must be cooled to a lower temperature than the pure solvent in order for freezing to occur. The freezing point of the solvent in a solution changes as the concentration of the solute in the solution changes (but it does not depend on the identity of either the solvent or the solute(s) particles (kind, size or charge) in the solution). The freezing point of the solvent in a solution will be less than the freezing point of the pure solvent whether the solution contains a non-volatile solute or a volatile solute. However, for simplicity, only non-volatile solutes will be considered here. SP. 10 Freezing Point total (Tb) = Freezing Point solvent (Tisolv) - AT, AT, = K,m where: AT+ = freezing point depression K+ = freezing point depression constant m = molality of solute constants for some common solvents: Solvent Water Benzene Chloroform Normal Freezing Point, °C 0.0°C 5.5°C -63.5°C Fp depression const., °C/mol 1.86 °C/mol 5.12 °C/mol 4.68 °C/mol Calculate the freezing point of a solution containing 4.27g of table sugar (C₁2H₂2011) in 50 g of water (H₂O).
SP. 11 Ethylene glycol is used as an anti-freeze in automoblie radiators. Determine the freezing point of 50% by weight solution of ethylene glycol, C₂H4(OH)2, supposing that ethylene glycol and water form an ideal solution. SP. 12. What is the freezing point of a solution prepared by adding 140. g trichothecin (C19H240s) to 0.746 kg of benzene?
Transcribed Image Text:SP. 11 Ethylene glycol is used as an anti-freeze in automoblie radiators. Determine the freezing point of 50% by weight solution of ethylene glycol, C₂H4(OH)2, supposing that ethylene glycol and water form an ideal solution. SP. 12. What is the freezing point of a solution prepared by adding 140. g trichothecin (C19H240s) to 0.746 kg of benzene?
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