Freezing Point Lab

Record your observations. Gently rinse your egg and find its mass. Record your data. Use the spoon to remove the egg from the beaker. Be EXTREMELY careful.

First, record the mass of two 150 mL beakers. Proceed to obtain a sample of unknown 3 and place about 2.5 to 3.0 g of the unknown into beaker 1 and record the mass. Slowly add 50 mL of distilled water into the beaker while stirring the mixture with a stirring rod. Prepare for gravity filtration by placing a funnel in an iron ring attached on a ring stand. Next, begin to fold a piece of filter paper, tearing off the corner of the smaller segment of the paper, and placing it in the funnel.

In an experiment similar to ours, after their data has been obtained, the enthalpy curve is calculated to be calculated (Haun, 2017). In our experiment, the freezing point of cyclohexane is 6.55 °C (Solvents, 2017). With trial two and three, we calculated the molarity and molality. For trial two, we had the molarity of 0.637160081 M and had the molality of 8.188m, which is provided below.

Jacob Winter Chem 101-103 11/7/16 Freezing Point Depression Introduction: The purpose of this lab experiment is to calculate the change in the freezing point of cyclohexanol and a solution made with cyclohexanol to find the molar mass of the unknown solute. The colligative properties of solutions are based on the concentration of molecules rather than the identity of the chemical. Freezing point, a colligative property of a solution, is constant in any substance and does not rely on the amount given.

Once the water is boiling, drop the metal into the pot and let it sit for 5 minutes. Place one Styrofoam cup into the other to craft a makeshift calorimeter. Measure the mass of the calorimeter. Then fill it ¾ of the way full with room-temperature water and measure the mass again.

The freezing point of water can vary. Adding substances, such as salt and sugar, can speed up or slow down the freezing point of water. Salt lowers the freezing point of water to below zero degrees Celsius, the initial freezing point of water. Lowering the freezing point of water is called Freezing Point Depression.

When the first ice crystals appear on the inside wall of the test tube, record the temperature. This should be the freezing point of the liquid. (In this step water is the pure solvent). Repeat as many times as necessary

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.

(Leave out the ice) Quickly, pour the hot and cold water into the beaker. Then stir the mixture of the hot and cold water. Place the temperature probe into the mixture.

To determine each solution's freezing point certain methods and materials were used. First, two weighing boats were labeled NaCl and CaCl2. Each weigh boat was placed on the scale to calculate the initial weight of the boats. 2.0g of sodium chloride was added to the boat labeled NaCl and reweighed. The same was done for CaCl2, then the freezing point apparatus was assembled. Using a 600mL beaker filled with ¾ full of ice, the remainder of NaCl was poured into the beaker and mixed. The thermometer was placed into the ice bath beaker until it became -10C. Four test tubes were labeled 1-4. For test tube 1, a 100mL graduated cylinder was used to measure 15mL of water and then poured into tube 1. After the temperature reached -10C, the thermometer

Apparatus and Method: The apparatuses you need for this experiment is a G clamp, Masses, Ring Stand and Newton meter. The Method: First hook the ring stand to the table using the G-Clamp Put the newton meter on the ring stand Make sure the newton meter is set on zero then hook 0.1 kg to the newton meter.

The melting point of a chemical is a physical property inherent to that substance. The chemical changes from a solid to a liquid state, but the composition remains the same. It can be used to determine the identity of an unknown substance. The purpose of this experiment was to discover the identity of an unknown chemical by determining its melting point.

After the water on the hotplate started to boil the metal was placed in the boiling water without touching the bottom or sides of the beaker. Then the Styrofoam cup was filled halfway with water and the mass was recorded. Then the temperature of the boiling water was measured with a probe that is plugged into a laptop which reads the temperature. After this the metal

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.

Throughout this experiment freezing point of water will be mentioned continuously so what is the freezing point exactly? The freezing point is the transition of when water turns to ice this happens at a certain temperature 32 degrees Fahrenheit or 0 degrees Celsius. “The typical freezing point of fresh water is 0° Celsius [32° Fahrenheit]. Generally, water molecules are composed of hydrogen and water molecules and they have bonded together into a crystalline structure ice.” (http://www.worldofchemicals.com/558/chemistry-articles/how-does-salt- lower- the-freezing-point-of-water.html, Data Research Analysis, 2017) This shows that when water turns to ice its a change in matter caused by the temperature. Which leads to why it can be altered because the temperature can always change and fluctuate. When a substance is added it can really take a toll on how the freezing point takes place. “While pure water freezes at 0°C (32°F), salt water needs to be colder before it freezes and so it usually takes longer to freeze. The more salt in the water, the lower the freezing point. Very salty water freezes at around -21 °C, or