Melting Ice Lab

The first part of the lab began by one lab member adding 10.0 mL of DI water to a test tube while another lab member obtained a beaker full of ice and salt. After both these steps were complete the test tube was put in the beaker full of ice. Immediately following the test tube be being placed in the beaker, a temperature probe was inserted into the test tube. The initial temperature was recorded and after the temperature was recorded in 30 second increments. Once the water exhibited supercooling and then remained consistent at .1 °C for 3 readings it was determined that the water had froze and formed crystals. Evidence that crystals formed allowed for it to be confirmed that the water actually hit freezing point at .0

Other substances that dissolve in water also lower the freezing point of the solution. The amount by which the freezing point is lowered depends only on the number of molecules dissolved, not on their chemical nature. This is an example of a colligative property. In this project, you'll investigate different substances to see how they affect the rate at which ice cubes melt. You'll test substances that dissolve in water (i.e., soluble substances), like salt and sugar, as well as substances that don't dissolve in water (i.e., insoluble substances), like sand and pepper. Which substances will speed up the melting of the ice?

From the excel chart of Molarity vs. Density, what was the relationship between the molarity of the sugar solution and the

40 g of ice and approximately 30 ml of sulfuric acid is cautiously added to a 100 mL beaker respectively. Weigh 7.6 g of ammonium chloride and 14.0 g of ammonium bromide and place it in another beaker, crushing the lumps until a powdery mixture remains. The powdery mixture is then transferred to a 125 mL Erlenmeyer flask. Add the ammonium salts into the sulfuric acid mixture. Heat is applied to dissolve the salt. Once the

Moisten filter paper with a few drops of solvent and turn on water vacuum to fullest extent

b. Place crushed ice in the beaker so the water level is just below the top of the

3. Do you think sugar or salt will melt at a higher temperature? Explain your answer.

1. Prepare the ice bowl by putting ice and water into a pan about 5 to 8 cm deep. Put 50 mL of chilled ethanol into the 100mL beaker and place the beaker in the ice bowl.

Attach your paperclip to your beaker, and lower your seed crystal into your solution (See Figure

After 5 min passed the plastic container created a thin layer of ice surrounding the container.

When adding a solute such as table salt or sugar to water, the resulting solution undergoes freezing-point depression. As a result of freezing-point depression, the solution results in an increase of entropy, which causes the boiling point of the solution to increase and the freezing point to

After that I waited until the entire ice cube melted. This took about two hours or so. Now that the ice had all melted and absorbed into the paper towel I could see that the ice cube had either broke through the paper towel, absorbed fully into the paper towel or leaked though in some spots. When I was finished looking over what had happened, I wrote down the results and everything all of my observations.

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

Materials: Observation 1; 1 cup of water, 2 cups of sugar, 1 glass jar, 1 wooden skewer, 1 plate and 2 clothespins. Observation 2; 1 cup of water, 3 cups of sugar, 1 glass jar, 1 wooden skewer, 1 plate, 5 drops of red food coloring, and one plate.

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