Wait a second!
More handpicked essays just for you.
More handpicked essays just for you.
Chemistry 101 lab
Don’t take our word for it - see why 10 million students trust us with their essay needs.
Recommended: Chemistry 101 lab
Objective: Making alum called potassium aluminum sulfate dodechydrate, from aluminum and potassium hydroxide. Materials: Aluminum foil weighing 1.0254 g ripped into small pieces, 250 mL beaker, Buchner funnel, filter paper, graduated cylinder, 25 Ml of 3 MKOH solution, Stirring rod, 35 Ml of sulfuric acid, 50 Ml of Aqueous ethanol solution. Procedure: we started this experiment by gathering aluminum foil, in the lab manual it does not clearly state how small the piece of foil need to be, so we cut them into about the size of tomato’s diced. The total weight of our foil was 1.024 g. Placed into a 250 mL beaker and 25 mL potassium hydroxide solution added with the foil. Once the solution was added we noticed a large amount of heat, and gas coming …show more content…
While the sulfuric acid was, being added we noticed a milky clump start to form, better known as precipitate but once the sulfuric acid was added completely instead the solution was thicker and cloudy white, sort of like the early starts of mashed potatoes. Our solution still had larger clumps of product so we decided to do the optional piece placed into our lab manual, which is filter the solution again to remove the clumps out. Once we filtered the solution for the total of 3 times during this lab we found that we had roughly 58 mL of solution left. This solution we took and placed on a hot plate to a slow boil until we reached 50 mL left the beaker. We then allowed the beaker to cool to room temperature and placed the beaker into the ice bath. During the ice bath, we ran into some issues after the 15 minutes had passed we had hardly any crystal formation, so by the advice of the professor we scraped the bottom and the sides of the beaker and left the beaker in the ice bath for an additional 10 minutes. Finally, we poured the crystal through a filter and poured 50 mL of ethanol solution over the crystals. Data: In the start of this lab we used aluminum foil weighing 1.0254 g, and the final weight of the product, 2KAl(SO4)2 * 12H20 + 3 H2 , was an actual yield of 6.3281 g. Once we finished this process we calculated the molar mass to find out the theoretical yield and the percent yield,
Each subsequent trial will use one gram more. 2.Put baking soda into reaction vessel. 3.Measure 40 mL vinegar. 4.Completely fill 1000 mL graduated cylinder with water.
Repeat for each trial. Rinse volumetric pipette with vinegar and drain into the waste beaker. Weigh and record the mass of each 200mL beaker. Add 10.00mL of vinegar into each beaker and weigh them and record their again. Add 50mL of de-ionized water to the beakers and place them under the drop counter on top of a stir plate, submerging the pH meter into the solution. Place the stir bar into the beaker and carefully turn on the stir plate so that the stir bar spins without splashing or hitting the sides of the beaker or the pH
The 100% theoretical yield should be 0.059 grams of myristic
To assemble this apparatus all of the following will be needed: a jacketed condenser, thermometer, 50 mL kjeldahl shaped flask, 100 mL kjeldahl flask, vacuum adapter, distilling column and a connecting adapter. Next, clamp the glass joints to the ring stand to properly secure the apparatus. Once finished with assembly, proceed to ad 60 mL of the fermented yeast prepared at the last experiment lab to the 100 mL flask and also add a small spin vane. Then, carefully place the flask into the sand bath. After this is done, let the water run that’s connected to the condenser slowly. At the same time, also slowly heat up the solution. For the experiment to be the most successful it’s important to slowly heat the flask because properly heating the flask will lead to a high percentage purity ethanol distillation. You can also add aluminum foil to the bottom of the flask, as this will help with the reflux process. Keenly observe the reflux process as you continue to slowly heat up the solution. Once the reflux line starts to get nearer to the connection adapter, record the temperatures. Once there’s a good amount of distillate in the 50 mL flask, go ahead and collect 2 to 3 mL of the distillate and transfer this into a labeled vial and give to your TA so he/she can measure out the distillate using a 1000 mL Eppendorf pipette. Lastly, weigh the solution on an analytical balance and record the weight. Using the weight recorded, calculate the density and compare to the density table listed below to determine the percent
While completing this lab we used four liquids. We used water, milk, orange juice, and soda. To hold the liquids we used two q-tips. We used two petri dishes, one was to hold the pill bugs while they were not being used in the
4. Pour about 300mL of tap water into the beaker. Set up a hot-water bath using a hot plate, retort stand, and thermometer clamp. Alternatively, use a Bunsen burner, retort stand, ring clamp, thermometer clamp, and wire gauze.
To properly complete this lab, a basic understanding of mass, moles, and empirical formula is required. Mass is a unit of measurement that is used to determine the number of grams in a certain object. A mole is a measurement in which the amount of substance that is present can be determined.To convert between from mass to moles the amount of grams present is divided by the atomic mass to find moles. To get back to mass from mols the amount of mols is multiplied by the atomic mass. An empirical formula is a chemical equation with the simpliest positive ratio possible. To find an empirical formula the elements in the formula must be in moles. Then the smallest amount of moles is used to divide all the other mole numbers. These numbers
== Refer to, Chemistry Lab #1 – What’s the substance? I didn’t change most materials when I did this experiment, but I added 4 materials, which are: * 5 test tubes * 2 stoppers * 1 large piece of paper And I deleted 1 material, which is: * Spatula Methods = == ==
== § Test tubes X 11 § 0.10 molar dm -3 Copper (II) Sulphate solution § distilled water § egg albumen from 3 eggs. § Syringe X 12 § colorimeter § tripod § 100ml beaker § Bunsen burner § test tube holder § safety glasses § gloves § test tube pen § test tube method = == = =
Analysis: This experiment is divided into two parts. In the first part; the standardized solution of sodium hydroxide is prepared by titrating it with base Potassium hydrogen phthalate (KHP). Phenolphthalein (range 8.3 to 10.0) is used as indicator to determine whether the titration is completed.
2. In the large beaker, put water and boil it completely. After that, remove the beaker from heat. 3. Sample tubes (A-D) should be labeled and capped tightly.
The lab we completed and the gold foil experiment are very similar in the ideas and ways that they worked. In the gold foil experiment the alpha-particle emitter would send a laser to bounce off a piece of gold foil which would cause some of the particles to be reflected and shown on the detecting screen. This is similar to the activity we completed because when we dropped the marble on the paper it acted as the laser, when the marble hit the carbon paper it was deflected onto the piece of circle paper underneath the carbon sheet. This activity and experiment contrasted because in the activity we completed there is not a similar size between the circles and the atoms. Atoms are the smallest unit of matter meaning that they are very hard to actually see, while in the
of distilled water. For the 1M solution I added 50 cm3 of HCl and 50
Add 15mL of 6N sulfuric acid to a 125mL Erlenmeyer flask containing 105mL of deionized water (preparing approximately 0.75N sulfuric acid). Obtain a sample of the unknown. Weight the vial and contents accurately on an analytical balance. Handle the vial with a small strip of paper to reduce the risk of error (due to added weight). Pour about half of the sample into a clean dry 200mL Erlenmeyer flask and weight again. Use the remaining half of the sample to get a second weight of around 0.6g-0.7g. Make sure the vial is capped on every weight taken.
0.1M HCl, 10 mL of 0.1N KMnO4, 0.2 g. KI, 5 mL of alcohol, and 5 mL of