Lab Report Of Freezing Point Of Cyclohexanol

In order to fulfil the labs purpose, the lab was split into two parts. The first part consisted of measuring and determining the freezing point depression of the solution water. The second part consisted of measuring and determining the freezing point depression of a solution that consisted of water and an unknown solute.

The freezing point depression constant for water that was experimentally determined in this analysis was 0.0479 °C/m, which was derived from the slope of the trend line in Figure 4. This is significantly lower than the constant stated in the literature of 1.86 °C/m.1 The freezing point temperature determined via cryoscopy should have been much lower in the high sucrose concentration solutions.

The freezing point constant (Kf) of water is 1.86 °C m-1. Each mass amount and Van’t Hoff factor was calculated then analyzed in a table.

The reaction "ICE" table demonstrates the method used in order to find the equilibrium concentrations of each species. The values that come directly from the experimental procedure are found in the shaded regions. From these values, the remainder of the table can be completed.

With time (t) on the x-axis and temperature (Celsius) on the y-axis, the exponential change could be easily observed. At the beginning of the laboratory the masses of the combined polypropylene test tube and 100 mL beaker were recorded by a digital electronic scale. A dry polypropylene test tube was obtained and approximately 2 mL of p-xylene was squirted into it with the use of a pipette. This was added to the beaker and weighed. 10 drops of toluene was then added and weighed again. The polypropylene test tube, which now contained 10 mL of p-xylene and 10 drops toluene was removed from the beaker and placed into a replica 100 mL beaker which was halfway filled with an ice water mixture. The temperature sensor, which was connected to the microlab application was placed inside of the polypropylene test tube and stirred rapidly around the outskirts of the bottom of the polypropylene test tube. The mixture began freezing, giving off an icy slush complex. Once the temperature appeared to have reached the nucleation point and leveled out at its freezing point, the application was stopped. This value was recorded in the laboratory manual. The temperature sensor was rinsed off then wiped, the beaker was re-filled with ice, and the test tube was put into the test tube rack to be thawed. Once thawed, this was discarded into the waste bin

Introduction: The experiment's goal was to determine the freezing point of a pure solvent and the freezing point depressions of two solutions. The freezing point and the freezing point depressions were determined by graphing the temperature of the pure solvent and two solutions as they cooled and observing when crystals first formed.

Purpose: The purpose of this laboratory was to gain an understanding of the differences between the freezing points of pure solvent to that of a solvent in a solution with a nonvolatile solute, and to compare the two.

This is done through the use of six different solutions. The first tube was only water and this was used to calibrate the temperature probe. This calibration determined that the freezing point of just water was -2.89°C. The other four tubes consisted of a sugar solution and the final tube consisted of a salt solution. For the sugar solution in tube two, 4.011g of sugar was used.

The graph for the freezing point of pure p-xylene turned out the way that was expected. As the p-xylene was stirred, a steep drop in temperature until reaching the trough of the graph around twenty-seven seconds. The temperature of the graph began slowly increasing as the p-xylene began to freeze until reaching the freezing point of the pure p-xylene in a process known as supercooling. The freezing point of the pure p-xylene was the point in which the temperature became level and steady. This point was at 13.974°C.

Many solutions can be used to lower the freezing point of water. They use salt to decrease the freezing point of water to keep roads clear of ice or other things that require decrease in waters freezing point. The colligative properties can be helpful in finding the molar masses of anonymous compounds. For low concentrations of substances that cannot be turned to gas readily, the freezing point depression of the solvent can be given in the

I. LIQUID - Identification of an Unknown Liquid: Using the physical properties of Solubility, Density, and Boiling Point.

The objectives of this lab are, as follows; to understand what occurs at the molecular level when a substance melts; to understand the primary purpose of melting point data; to demonstrate the technique for obtaining the melting point of an organic substance; and to explain the effect of impurities on the melting point of a substance. Through the experimentation of three substances, tetracosane, 1-tetradecanol and a mixture of the two, observations can be made in reference to melting point concerning polarity, molecular weight and purity of the substance. When comparing the two substances, it is evident that heavy molecule weight of tetracosane allowed

The purpose of this experiment was to identify any possible relationship between salts and freezing point depression by testing their effects on the temperature of an ice cream mixture.

It is suspected that the freezing point is 64.1oC. Due to the short temperature plateau, It is difficult to determine if the freezing point occurs at during the interval (6:00-6:10). However, it appears to be have been the most reasonable determination for freezing point in comparison to the rest of the plot.

As stated, our solvent in this lab will be tert-butanol. We start by recording the freezing point of this substance without anything added. Then, we add various