Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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**Boiling Point Elevation/Freezing Point Depression** \[\Delta T = m \cdot K\] where, for freezing point depression: \[\Delta T = T(\text{pure solvent}) - T(\text{solution})\] and for boiling point elevation: \[\Delta T = T(\text{solution}) - T(\text{pure solvent})\] - \(m\) = (# moles solute / Kg solvent) - \(K_b\) = boiling point elevation constant. - \(K_f\) = freezing point depression constant. \(K_b\) and \(K_f\) depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. | Solvent | Formula | \(K_b\)(°C / m) | \(K_f\)(°C / m) | |--------------|---------------|------------------|------------------| | Water | H₂O | 0.512 | 1.86 | | Ethanol | CH₃CH₂OH | 1.22 | 1.99 | | Chloroform | CHCl₃ | 3.67 | | | Benzene | C₆H₆ | 2.53 | 5.12 | | Diethyl ether| CH₃CH₂OCH₂CH₃ | 2.02 | |
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Transcribed Image Text:**Boiling Point Elevation/Freezing Point Depression** \[\Delta T = m \cdot K\] where, for freezing point depression: \[\Delta T = T(\text{pure solvent}) - T(\text{solution})\] and for boiling point elevation: \[\Delta T = T(\text{solution}) - T(\text{pure solvent})\] - \(m\) = (# moles solute / Kg solvent) - \(K_b\) = boiling point elevation constant. - \(K_f\) = freezing point depression constant. \(K_b\) and \(K_f\) depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. | Solvent | Formula | \(K_b\)(°C / m) | \(K_f\)(°C / m) | |--------------|---------------|------------------|------------------| | Water | H₂O | 0.512 | 1.86 | | Ethanol | CH₃CH₂OH | 1.22 | 1.99 | | Chloroform | CHCl₃ | 3.67 | | | Benzene | C₆H₆ | 2.53 | 5.12 | | Diethyl ether| CH₃CH₂OCH₂CH₃ | 2.02 | |
The freezing point of water is 0.00 °C at 1 atmosphere. *Problem Statement:* How many grams of calcium nitrate (164.1 g/mol) must be dissolved in 218.0 grams of water to reduce the freezing point by 0.350 °C? Refer to the table for the necessary boiling or freezing point constant. *Data Table:* - **Solvent:** Different solvents and their properties - **Formula:** Chemical formula of each solvent - \( K_b \) \((\degree C/m)\): The boiling point elevation constant for each solvent - \( K_f \) \((\degree C/m)\): The freezing point depression constant for each solvent | Solvent | Formula | \( K_b \) \((\degree C/m)\) | \( K_f \) \((\degree C/m)\) | |----------------|--------------------|-----------------------------|-----------------------------| | Water | \( \text{H}_2\text{O} \) | 0.512 | 1.86 | | Ethanol | \( \text{CH}_3\text{CH}_2\text{OH} \) | 1.22 | 1.99 | | Chloroform | \( \text{CHCl}_3 \) | 3.67 | | | Benzene | \( \text{C}_6\text{H}_6 \) | 2.53 | 5.12 | | Diethyl ether | \( \text{CH}_3\text{CH}_2\text{OCH}_2\text{CH}_3 \) | 2.02 | | The task is to calculate the mass of calcium nitrate needed using the properties of water from this table: \( K_f = 1.86 \degree C/m \). **Mass = \(\boxed{\phantom{g}}\)**
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Transcribed Image Text:The freezing point of water is 0.00 °C at 1 atmosphere. *Problem Statement:* How many grams of calcium nitrate (164.1 g/mol) must be dissolved in 218.0 grams of water to reduce the freezing point by 0.350 °C? Refer to the table for the necessary boiling or freezing point constant. *Data Table:* - **Solvent:** Different solvents and their properties - **Formula:** Chemical formula of each solvent - \( K_b \) \((\degree C/m)\): The boiling point elevation constant for each solvent - \( K_f \) \((\degree C/m)\): The freezing point depression constant for each solvent | Solvent | Formula | \( K_b \) \((\degree C/m)\) | \( K_f \) \((\degree C/m)\) | |----------------|--------------------|-----------------------------|-----------------------------| | Water | \( \text{H}_2\text{O} \) | 0.512 | 1.86 | | Ethanol | \( \text{CH}_3\text{CH}_2\text{OH} \) | 1.22 | 1.99 | | Chloroform | \( \text{CHCl}_3 \) | 3.67 | | | Benzene | \( \text{C}_6\text{H}_6 \) | 2.53 | 5.12 | | Diethyl ether | \( \text{CH}_3\text{CH}_2\text{OCH}_2\text{CH}_3 \) | 2.02 | | The task is to calculate the mass of calcium nitrate needed using the properties of water from this table: \( K_f = 1.86 \degree C/m \). **Mass = \(\boxed{\phantom{g}}\)**
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