The Formation of Alum Crystals from Solutions in Different Thermal Conditions

Next, 1mL plus an additional 10 drops of 10% sodium carbonate was added drop-wise to the beaker until the solution reached a pH of 8. The precipitate formed (crude benzocaine product) was collected via vacuum filtration and washed with water during the transfer into the Hirsch funnel. The product was allowed to dry for one week after which the mass and melting point of the crystals were measured.

The mixture was transferred to an ice bath to crystallize the product, after which the product was collected by vacuum filtration on a Hirsch funnel, washing the flask with small aliquots of cold xylene and pouring the solution over the crystals, allowing the vacuum to thoroughly dry the product. Additional drying was achieved by transferring the product to filter paper and pressing the crystals to remove any excess moisture. The product was then weighed and a melting point determined. A comparative TLC was run in Hexanes:Ethyl Acetate solvent against maleic anhydride to verify the purity of the

Have you ever seen a sugar crystal before? Or how does sugar turn into crystals? At what temperature do crystals form? Or does the temperature affect the growth of crystals forming? This is the type of question you really do not ask yourself. But for the sake of science, we had to find out the right temperature in which the crystals will form. Sugar crystals go through a chemical reaction in which it separates one compound from the others or vice versa. The sugar crystals goes through this process of crystallization and supersaturation. It shows how there is an excess amount of sugar in the sugar vs. the water ratio as the water is gradually evaporating. You could benefit by this by observing through time of how the water of the sugar crystals

The product was placed in a Craig tube and several drops of hot (100°C) solvent (50% water, 50% methanol, by volume) was added and heated until all of the crystals dissolved. The Craig tube was plugged and set in an Erlenmeyer flask to cool. Crystallization was induced once the mixture was at room temperature by scratching the inner wall of the tube. It was then placed into an ice bath for ten minutes until crystallization was complete. The tube was then

The first step is the separation of the solid crystals back into separate ions, a positive ammonium ion and a negative nitrate ion. The break these ionic bonds requires a lot of energy which means heat must be taken from the surrounding water. The second step the water molecules, which are H2O, are attracted to the ions and attach themselves to the ions. The second step actually causes heat to be produced to the surrounding liquid mixture. .Even

21) After all of the solid dissolves, move the flask from the hot plate and allow it cool to room temperature. After a while, crystals should appear in the flask.

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

An unknown compound was obtained and the ID number was recorded. A capillary tube was loaded with the unknown powder and inserted into the melting apparatus. The temperatures at which the crystals first started to liquefy and when the entire sample became liquid were recorded. The melting point was then compared with previous known mixture samples to identify the unknown compound.

To achieve the goals set forth for this laboratory experiment, the green crystals first needed to be constructed. Using the Dial-O-Gram, 8.3 grams of K2C2O4 H2O was collected and placed into a 125 mL flask. Following that step, 25 mL of deionized water was added to the same flask and the solid substance was alloted time to dissolve. Once this was completed, 4.1g of FeCl3 6H2O was collected using the Dial-O-Gram and placed into a 150 mL beaker. To aid in the dissolving of the solid, 10 mL of DI water was added to the beaker.

For the Synthesis of Alum lab my lab group and I took 1 gram of aluminum foil and broke it into small pieces. Next we added 25 mL of 3M KOH solution. Once the foil was dissolved we filtered the solution through a Buchner funnel with filter paper sealed inside with water. As the solution was filtering we applied a vacuum filtration to the Buchner funnel to expedite the filtering process. Once it was completely filtered my lab group poured the solution into a beaker and covered the beaker with parafilm. We then waited overnight to allow the crystals to form inside the beaker. Unfortunately, we did not produce any crystals overnight so we borrowed some from another group. Once we obtained the crystals we had to stir them in a beakers to make more form other than just the ones we received. After we rinsed the crystals with half ethanol and half water mixture. Once they were dry we determined the mass of the crystals with a balance.

April 2000, the largest gypsum crystal in the world are found in Naica Mexico mine’s Cave of Crystals. Crystals can be made in many different ways. Earth can either make them or they can be made artificially. Crystals can be made out of salt or borax. The earliest crystal grower was Earth. For salt crystal the water starts to evaporate the solution of the amount of salt in the glass that it remains the same. There is not enough water left to keep the sodium and chlorine ions from joining together (What Controls Crystal Growth?). Salt crystals are formed. This experiment will conduct of the type of water will affect the growth of crystals.

The mixture was cooled to room temperature and 40mL of of water was added. The stopper was placed on the flask and shaken until the liquid residue solidified. After the product solidified, the flask was placed in an ice bath and the solid was was broken up with a string rod until it was a fine powder. The product was then collected by vacuum filtration and was washed three time with 5-mL of cold water then left to dry.

Hydrates are a crystalline compound. A hydrate is formed when water molecules are chemically blended with another compound or element. A crystalline compound is any formation of molecules, ions, or atoms that are joined together in a 3-dimentional formation. A crystalline structure is one of the 2 types of ordering atoms. The bond that holds the salt and water together is not very strong. Therefore, it is easy to separate it. The hydrate has weak bonds because of the ionic nature of salt and the polarity of water. To separate the water and salt, the hydrate must be heated. This will evaporate the water, thus leaving the salt. The left-over salt in the container is called the anhydrous salt. Anhydrous is the term that is used to explain that

Crystals were collected in a Buchner funnel, washed with alcohol, then ether, then transferred into a sample tube for storage.

Add 10 mL of 95% ethanol to the beaker and warm it in a water bath in order to dissolve the crystals