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Assuming 100% dissociation, calculate the freezing point and the boiling point of 0.570 mol K3PO4 in 1.00 kg water. You may need the colligative constants for water.

Assuming 100% dissociation, calculate the freezing point and the boiling point of 0.570 mol K3PO4 in 1.00 kg water. You may need the colligative constants for water.

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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Assuming 100% dissociation, calculate the freezing point and the boiling point of 0.570 mol K3PO4 in 1.00 kg water. You may need the colligative constants for water.

### Colligative Constants Below are constants for freezing-point depression and boiling-point elevation calculations at 1 atm: | Solvent | Formula | \( K_f \) Value* (\( °C/m \)) | Normal Freezing Point (°C) | \( K_b \) Value (\( °C/m \)) | Normal Boiling Point (°C) | |------------------|-----------|-------------------------------|-----------------------------|------------------------------|---------------------------| | Water | H\(_2\)O | 1.86 | 0.00 | 0.512 | 100.00 | | Benzene | C\(_6\)H\(_6\) | 5.12 | 5.49 | 2.53 | 80.1 | | Cyclohexane | C\(_6\)H\(_12\) | 20.8 | 6.59 | 2.92 | 80.7 | | Ethanol | C\(_2\)H\(_6\)O | 1.99 | -117.3 | 1.22 | 78.4 | | Carbon Tetrachloride | CCl\(_4\) | 29.8 | -22.9 | 5.03 | 76.8 | | Camphor | C\(_10\)H\(_16\)O | 37.8 | 176 | - | - | **Explanation:** - **\( K_f \) and \( K_b \) Values:** These are constants used to calculate the freezing-point depression and boiling-point elevation, respectively, for solutions. - **Normal Freezing and Boiling Points:** These values indicate the temperatures at which the solvent will freeze or boil at 1 atmosphere of pressure. Understanding these constants is essential for predicting how the presence of solutes will affect the physical properties of solutions.
Transcribed Image Text:### Colligative Constants Below are constants for freezing-point depression and boiling-point elevation calculations at 1 atm: | Solvent | Formula | \( K_f \) Value* (\( °C/m \)) | Normal Freezing Point (°C) | \( K_b \) Value (\( °C/m \)) | Normal Boiling Point (°C) | |------------------|-----------|-------------------------------|-----------------------------|------------------------------|---------------------------| | Water | H\(_2\)O | 1.86 | 0.00 | 0.512 | 100.00 | | Benzene | C\(_6\)H\(_6\) | 5.12 | 5.49 | 2.53 | 80.1 | | Cyclohexane | C\(_6\)H\(_12\) | 20.8 | 6.59 | 2.92 | 80.7 | | Ethanol | C\(_2\)H\(_6\)O | 1.99 | -117.3 | 1.22 | 78.4 | | Carbon Tetrachloride | CCl\(_4\) | 29.8 | -22.9 | 5.03 | 76.8 | | Camphor | C\(_10\)H\(_16\)O | 37.8 | 176 | - | - | **Explanation:** - **\( K_f \) and \( K_b \) Values:** These are constants used to calculate the freezing-point depression and boiling-point elevation, respectively, for solutions. - **Normal Freezing and Boiling Points:** These values indicate the temperatures at which the solvent will freeze or boil at 1 atmosphere of pressure. Understanding these constants is essential for predicting how the presence of solutes will affect the physical properties of solutions.
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