Carbohydrates- In this experiment We test for starch. We pour drops of Iodine onto the different liquids. If starch is present the liquid is to turn a blue/black color. Lipids- In this experiment we are testing for lipids. We pour a drop or two of water onto one piece of paper bag and another drop of oil onto a different piece of paper bag.
Biuret solution tests protein a. Use a stir stick to put a small drop of EACH food from the test tube into a different well in the Well plate b. Add a drop of Biuret solution to each well. c. Record any color changes. 5.
Halides Lab: Background information: Halide ions are reactive and useful. Salts are positively charged ions (metals) combined with any negative ions (nonmetal), and when placed in a solution (water) it separates into the cations and anions that made it up. The Purpose of this lab is to find out how the Halides react with the indicators, and to determine the identity of the two unknown solutions (A and B). Color of solutions prior to experiment: NaF | NaCI | KBr | KI | Unknown A | Unknown B | clear | clear | clear | clear | clear | clear | Color of indicator prior to experiment: 5% Bleach (NaOCI) | 0.2 M Na2S2O3 | 0.1 M AgNO3 | 0.5 M Ca(NO3)2 | clear | clear | clear | clear | Halide solutions | NaF | NaCI | KBr | KI | unknown A | unknown B | Test 1: Ca(NO3)2 | Cloudy White (Nothing) | Clear | Nothing | light yellow (Nothing) | Nothing | Nothing | Test 2, Part A: AgNO3 | clear (Nothing) | Milky White | Gold (Cloudy yellow) | milky green (Cloudy yellow) | turned white, film developed on top layer | Milky | Test 2, Part B: add Na2S2O3 to test tube from part A | Dark Orange/brown | Clear | Dark Gold(precipitate yellow then clear) | milky green (no change) | white precipitation, settled on bottom | Milky | Test 3: NaOCI (Bleach) | Clear (Nothing) | Nothing | Nothing | Orange (Clear) | Nothing | Orange | Unknown A is identified as NaCI (Sodium Chloride), because in test#1 the solution turned a cloudy white color when Ca(NO3)2 (Calcium nitrate) was added. In the first part of test#2, when AgNO3 (Silver nitrate) is added, the solution turned white, with a thin layer of film developing on the surface.
The test for Sodium Bicarbonate included mixing that with HCl. After doing this experiment bubbles would form in the solution. This was CO2 being released. This reaction is a way of testing for Sodium Bicarbonate. BACKGROUND: For these experiments a 96-well plate was used.
Copper (II) sulfate is a bright shade of blue, and very toxic to the environment, irritating to the eyes and skin, and also can cause damaging effects if swallowed. The lab involved calculations with mole ratios, the mass of water, and comparing the actual and theoretical masses. Also this lab dealt with determining the mass of the compound before and after heating had occurred. PURPOSE The purpose of this lab is to determine the mass of water that is contained in a sample of a hydrate of copper(II)sulfate MATERIALS •large test tube •utility clamp •iron stand •bunsen burner •flint lighter •balance •hydrated copper(II)sulfate •stirring rod PROCEDURE 1. The mass of a clean dry test tube was accurately measured.
Based on the handbook, the color of the iodine should be violet black, which was one of the properties I observed. It is soluble in alcohol, mineral oil, and potassium iodide and insoluble in water. I obtained the same results although for some substances more iodine dissolved than others. This could have been because perhaps we used too big pieces of solid iodine. If there wasn’t enough solution to react with it then that would explain why we still had some left over that didn’t.
It is known that chlorine is more electronegative than bromine, and thus chlorine is more reactive, and less discriminatory as to what it will react with, thus making bromine more “selective”. Another pertinent piece of information to look at would be stability. The stability of a free radical increases as the number of carbon substituents increases. Therefore, primary is the least stable and tertiary is the most stable. Also, the more stable the free radical that is left behind, the weaker its C-H bond strength will be.
Compare the efficiencies of the two distillation methods in your lab notebook. Postlab questions: 1,3 on p. 65. Please include the answers in the appropriate section of your lab report. (Results and Discussion or Conclusions) Sept. 11-17 Prelaboratory
O O O O O O O O I I I O O O O O O I O O O I I O The top three are equally important. The first two on the bottom are of equal importance. I think the bottom right two will be most important (fewer formal charges), then maybe the bottom left structure (maximize bonding), then the top three structures. The order of importance isn’t entirely clear between the last two groups. (Argument between maximize bonding and put negative charge on the more electronegative atom.)
Observations of Physical and Chemical Changes Purpose- The different tests can interact and change in different ways, by doing these tests we can figure out if it could be either a physical change or chemical change by observing the test and chemicals. Procedure- In test one, you mixed a small amount of iodine in each test tube and fill one of the with just tap water and the second one with hexane. Test two, you measure 5 grams of barium hydroxide and same measurement of ammonium chloride and stir with a stirring rod. Test three, you use a small piece of steel wool and you place it over a Bunsen burner using tongs and observe what you see. Test four, by using a plastic bag, you place a spoon full of calcium chloride in one corner and