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Colligative properties represent the changes in the physical properties of a solution that result from the addition of a non-volatile solute to a solvent. These changes, which include alterations in vapor pressure, freezing point depression, and boiling point elevation, are dependent on the quantity of solute particles but are independent of their nature. This investigation focuses on freezing point depression, a colligative property where the addition of a solute to a solvent decreases the temperature at which the solvent freezes.
By examining the freezing point depression of naphthalene solutions with known and unknown solutes, we aim to elucidate the principles governing colligative properties and calculate the molar mass of an unknown solute.
The primary goal is to explore how the introduction of a non-volatile solute affects the freezing point of a solvent and to apply this understanding to determine the molar mass of an unknown solute.
Protective equipment including goggles, lab coats, and proper footwear were worn throughout the experiment to ensure safety.
The freezing point depression was used to calculate the molality of the solutions, which was then applied to determine the molar mass of the unknown solute, p-nitrotoluene.
| Naphthalene | Naphthalene + 1,4-
dichlorobenzene |
Naphthalene + p-nitrotoluene | |||
| Initial
temperature |
90 | Initial
temperature |
85 | Initial
temperature |
85 |
| Time (sec) | Temp (ºC) | Time (sec) | Temp (ºC) | Time (sec) | Temp (ºC) |
| 30 | 84.0 | 30 | 80.0 | 30 | 76.0 |
| 60 | 82.0 | 60 | 79.0 | 60 | 70.0 |
| 90 | 80.5 | 90 | 78.5 | 90 | 69.0 |
| 120 | 80.5 | 120 | 76.0 | 120 | 68.5 |
| 150 | 80.0 | 150 | 75.5 | 150 | 68.0 |
| 180 | 80.0 | 180 | 75.0 | 180 | 68.0 |
| 210 | 80.0 | 210 | 75.0 | 210 | 68.0 |
| 240 | 80.0 | 240 | 75.0 | 240 | 68.0 |
| 270 | 79.5 | 270 | 74.5 | 270 | 67.0 |
| 300 | 78.5 | 300 | 74.0 | 300 | 64.0 |
| 330 | 78.0 | 330 | 73.0 | 330 | 63.5 |
| 360 | 73.0 | 360 | 68.0 | 360 | 63.5 |
| 390 | 68.0 | 390 | 66.0 | 390 | 63.0 |
| 420 | 65.5 | 420 | 64.0 | 420 | 62.5 |
| 450 | 62.5 | 450 | 63.0 | 450 | 62.5 |
| 480 | 61.5 | 480 | 62.5 | 480 | 61.0 |
| 510 | 60.0 | 510 | 60.0 | 510 | 60.0 |
The experiment yielded precise measurements of the freezing points for pure naphthalene and its solutions with known and unknown solutes.
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The analysis revealed the expected decrease in freezing points for the solutions compared to the pure solvent, illustrating the impact of solute addition on colligative properties.
The observed freezing point depressions align with the theoretical expectations outlined by colligative property principles. The presence of solute particles in the solvent reduces its ability to form a solid at its normal freezing point, necessitating a lower temperature to achieve solidification. This effect was quantitatively analyzed using the relationship between freezing point depression, molality of the solution, and the molar mass of the solute, leading to the determination of the molar mass of p-nitrotoluene.
Potential sources of error include inaccuracies in temperature measurements and solute mass, which could be minimized with more precise instrumentation and measurement techniques. Additionally, ensuring a homogeneous solution and preventing supercooling are crucial for accurate determination of freezing points.
This investigation into the colligative properties of solutions, specifically freezing point depression, has provided valuable insights into the effect of solute addition on solvent behavior. By meticulously measuring the freezing points of naphthalene solutions with both known and unknown solutes, we successfully determined the molar mass of an unknown solute, demonstrating the practical application of colligative property principles in analytical chemistry.
Understanding Colligative Properties through Freezing Point Depression. (2024, Feb 26). Retrieved from https://studymoose.com/document/understanding-colligative-properties-through-freezing-point-depression
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