AP Chemistry P2 Experiment 2: Formula of a Hydrate 9/24/2013 Purpose: Calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate. Procedure: 1) Set up ring stand with ring clamp, clay triangle, crucible with lid, and burner. Adjust the height of the ring stand. 2) Dehydrating Procedures: 3. Measure approximately 1 g of Copper(II) Sulfate Hydrate into the crucible and crucible and lid.
Add the HCl SLOWLY to the magnesium by running it down the side of the beaker. Adding the acid too quickly will result in the spattering of the acid. Write down any observations of the reaction. 6. After all the acid has been completely added and the reaction has stopped, use a pipette to add a few extra drops of acid into the beaker until the reaction stops.
Observe the color change while it is being heated. After observing the color change, find the mass and moles of the hydrate. Then find the mass and moles of the water eliminated. And lastly find the mole ratio of water to hydrate. For part 2, do the same thing as part 1 except use an unknown hydrate and calculate the percent mass of water in an unknown hydrate.
Lab 4: Determination of Percent by Mass of the Composition in a Mixture by Gravimetric Analysis Introduction Thermal gravimetric analysis is used to determine the percent by mass is used to determine the percent by mass of a component in a mixture. When a mixture is heated to an appropriately high temperature, one component in the mixture decomposes to form a gaseous compound. The mass of this particular component is related to the mass of the gaseous compound. In this experiment, the percent by mass of sodium hydrogen carbonate (NaHCO3) and potassium chloride (KCl) in a mixture will be determined. Experimental First, we weighed 2 samples, each has 1 gram of NaHCO3-KCl mixture Second, we put the samples in 2 crucibles (A and B) and weighed them.
Directions: Follow the directions for the volcano, but use more of the sweets to create a bigger explosion. Warning: Certainly do not try this indoors as this will create a huge mess. Soda and Mentos Rocket For this experiment you will need a lot of space and an area where the rocket will not land on anybody or anything; a park is the ideal place. Directions: Remove the lid from the soda and the outer paper wrapper from the tube of Mentos--but do not remove the inner foil wrapper. Put the entire tube in the bottle and replace the cap.
Then by writing a balanced chemical equation and using the titration formula, Nb+Ma+Va=Na+MbVb , the molarity is able to be determined. Procedure: 1) Using the graduated cylinder add 10.0 mL of water into the Erlenmeyer flask. 2) Add 5.0 mL of HCl into the flask using another graduated cylinder because acid goes into water when mixing them. 3) Add three drops of phenolphthalein indicator into the flask. 4) Swirl the flask in circular movements to mix the substances.
After 10 seconds, the colorless mixture suddenly turns blue. Concept: Demonstrates a typical clock reaction; shows the effect of the interaction between chemical reactions that have different rates. Materials: • Solution A o 0.6 grams Starch o 30 mLs of Acetic Acid o 4.1 grams of Sodium Acetate o 50 grams of Potassium Iodide o 4.7 grams of Sodium Thiosulfate ▪ Allow mixture to cool and dilute to 1 liter with distilled water o 1 liter flask • Solution B o 500 mLs of 3% Hydrogen Peroxide o 500 mLs of distilled water o 1 liter flask o Safety: Hydrogen Peroxide can be irritating to skin and eyes. Wear safety goggles and gloves. Procedure: Mix the two solutions together.
Task 3 To separate a mixture containing water (boiling point 100 0C) butan-1-ol (boiling point 117 0C) I will use fractional distillation. I am choosing fractional distillation as it is the process by which components in a chemical mixture are separated according to their different boiling points . Vapors from a boiling solution are passed along a column. The temperature of the column gradually decreases along its length. Components with a higher boiling points condense on the column and return to the solution ; components with a lower boiling points pass through the column and are collected.
It dehydrates sucrose (table sugar), C12H22O11, leaving a spongy black mass of carbon and diluted sulfuric acid. Concentrated sulfuric acid reacts similarly with skin, paper, and other animal and plant matter. When it is mixed with water, a highly exothermic reaction occurs, and the energy released can be enough to heat the mixture to boiling. Therefore, concentrated sulfuric acid has to be diluted by adding the acid slowly to cold water while the mixture is stirred to dissipate the heat. The first successful method for making sulfuric
Using a measuring cylinder, pour 20 cm3 of 0.01M saturated cobalt (II) chloride solution at 0℃ and pour about 100 cm3 of deionized water to a 250 cm3 beaker. 2. Stir the mixture using a magnetic stirrer-hotplate. 3. Using a dropper, add 5 drops of concentrated hydrochloric acid to the solution.