# Colligative properties lab report. Lab report_ Colligative Properties, Freezing Point childhealthpolicy.vumc.org 2022-10-19

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Colligative properties are properties of solutions that depend on the concentration of solute particles, but not on the identity of the solute. These properties include boiling point elevation, freezing point depression, osmotic pressure, and vapor pressure lowering.

In a colligative properties lab, students may be asked to measure the boiling point elevation or freezing point depression of a solution and compare it to the expected value calculated using the appropriate colligative property equation. For example, to measure the boiling point elevation of a solution, a student may prepare several solutions of different concentrations and use a thermometer to measure the boiling point of each solution. The student can then compare the measured boiling points to the expected values calculated using the equation for boiling point elevation, which is:

ΔTb = Kb * molality

Where ΔTb is the boiling point elevation, Kb is the boiling point elevation constant for the solvent, and molality is the concentration of the solute in molality (moles solute per kilogram solvent).

Another common colligative property experiment involves measuring the osmotic pressure of a solution. Osmotic pressure is the pressure that must be applied to a solution to prevent the flow of solvent into the solution across a semi-permeable membrane. To measure osmotic pressure, a student may prepare several solutions of different concentrations and use a manometer to measure the pressure required to prevent the flow of solvent into the solution. The student can then compare the measured osmotic pressure to the expected value calculated using the equation for osmotic pressure, which is:

Π = M * R * T

Where Π is the osmotic pressure, M is the concentration of the solute in moles per liter, R is the ideal gas constant, and T is the temperature in kelvin.

In addition to measuring colligative properties, a colligative properties lab may also include an investigation of the relationship between colligative properties and molality. For example, students may be asked to plot the boiling point elevation or freezing point depression of a solution as a function of molality and observe the linear relationship between these properties.

Overall, a colligative properties lab provides students with the opportunity to explore the properties of solutions and understand how they are affected by the concentration of solute particles. This understanding is important for a variety of applications, including the purification of substances, the formulation of medications, and the design of industrial processes.

## Freezing point depression lab report

If one can count the number of moles of a substance in a given number of grams of that substance, the molar mass is easily calculable. This phenomenon is closer to ideal in dilute solutions rather than concentrated ones. To understand osmotic pressure, it is helpful to know the basics of osmosis. Background: Colligative properties are properties of a solvent, such as freezing point depression and boiling point elevation, which depend on the concentration of solute particles dissolved in the solvent. The error for the molar mass of ethylene glycol for this experiment was found to be 37%. The ions split into positives and negatives and produce multiple ion particles.

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## Lab #6 Colligative Properties: Freezing Point Depression and Molar Mass Flashcards

Once the temperature of the t -butanol has warmed to about 40 °C, transfer the test tube to the ice- water bath making sure that most of the t -butanol is below the surface of the ice-water bath, add more ice if needed. They are the affected properties when a nonvolatile solute is added to a solvent. An example of a cooling curve is shown below in Figure 1. Clean-Up: Place the test tube back in the warm water bath to melt the solid. Osmotic flow is from a solvent to a solution. Molar solubility is defined as the amount in moles of solute per liter of saturated solution. CHEM 1002 COLLIGATIVE PROPERTIES Laboratory Report A.

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## Colligative Properties Lab Report

As the sample begins to solidify the change in temperature will slow, and at the equilibrium shown by Eq 7 the temperature will be constant until all of the sample has solidified. Remove the thermometer and stirring loop. Student 14 1 14. Show all calculations and report the molar mass of unknown as determined in each of the two solutions. Each solute has a different curve. For example, ionic solutes dissolve and split when placed in a solution.

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## Lab Report On Colligative Properties

Place the beaker with test tube on a top loader balance and tare the balance. Less solute causes a lower boiling point. The more solute, the higher the boiling point. Do not try to pull the thermometer and stirrer from the frozen t -butanol! This is most easy to see in cooking pasta in boiling water with salt. From that calculation of molar mass, one is expected to be able to perform error analysis by comparing experimentally obtained values for molar mass to a given molar mass for an organic substance.

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## Non Colligative Properties Lab Report

Student 16 1 14. Angue Group 4 - Enthalpy Date experiment performed: November 16, 2022 Wednesday Colligative Properties of a Solution The ratio of solute to solvent particles determines how well-coordinated a solution is. When more particles are added to the solution, the vapor pressure is low, the boiling point increases and the freezing point decreases. With a disposable pipette add about another 0 g of the unknown to the test tube and record the mass, line 5 this is sample solution 2. To construct a cooling curve one would warm their sample, pure solvent or solution, to well above its melting point, then allow it to cool.

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## Colligative properties

Examples are shown in Figure 1. This also raises the boiling point and lowers the freezing point. This affected the overall readings. These properties are properties that are affected when a solute is added to a solvent. When a non-volatile does not vaporize solute mixes with the solvent, it lowers the vapor pressure of the solvent.

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## Colligative Properties Lab report

Clearly mark on each graph all your data points and the best fit lines you used to determine each freezing point. Thus, molarity, normalcy, and molality are only a few of the parameters that may be used to indicate the concentration of a solution together with colligative qualities. Use the information to determine the molar mass of your unknown substance. CHEM 126 LAB February 17th 2021 Experiment 3: Colligative Properties Introduction: Colligative properties are a properties that depends on the number of particles dissolve in solution and not on the identity of the identity of species. Colligative properties do not depend on the IMF PRESENT. Lowering the vapor pressure will in turn increase the boiling point, as there is more energy needed to cause the solvent to vaporize. If you need more ice for your ice- water bath get it.

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## Lab report_ Colligative Properties, Freezing Point childhealthpolicy.vumc.org

Osmosis is when molecules of a solvent pass through a semipermeable membrane to the more concentrated side of a u-tube. There are 2 equations use to find kb and kf of solutions 1. Colligative Properties: Freezing Point Depression Experiment 4 Abstract In lab, we did an experiment to understand the concept of colligative properties. Cyclohexane Trial 1 Lab 1: Colligative Properties Cyclohexane trial 2 B. Student 12 1 14.

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## Colligative Properties lab report childhealthpolicy.vumc.org

Because of the salt, the water will boil at a higher temperature, which in turn causes the noodles to cook faster. This student was allowed to give oral responses to written responses on assessment, but then was also be encouraged to attempt to write responses as well. Conclusion The experiment was successful. Large sources of error were found because the ethylene glycol used was antifreeze. A depression of the solvent freezing point occurs. Colligative properties are useful in counting moles of solute, even when the identity of the solute is not known.

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