Detecting Signs of Chemical Change Abstract: The objective of this experiment will be to combine various substances, liquids and metals, and to observe their behavior when they are combined. The types of reactions observed shall determine the nature of these reactions: physical or chemical. Introduction: An elements¡¦ reaction to certain substances may be predicted by its placement on the Periodic Table of Elements. Across a period, an element on the left will react with more vigor than one on the right, of the same period. Vertically, as elements are sectioned into groups, the reaction of each element increases as you move down in the same group. With this in mind, the reactions of the substances involved in this experiment may be hypothesized, observed, and validated. Material and equipment: X 12 test tubes X 10-mL graduated cylinder X Water ¡V deionizer (distilled water) X 0.1M cobalt (II) chloride hexahydrate X 95% ethanol X 0.1M cobalt (II) chloride hexahydrate dissolved in 95% ethanol X zinc X 1M hydrochloric acid solution X 0.1M copper (II) sulfate solution X 0.5M sodium hydrogen carbonate solution X 1M ammonia solution X magnesium X 1M sodium hydroxide solution X ammonium chloride Procedure: A. Be sure to always start with clean, dry test tubes, equipment, and tools. B. Put a label on each test tube. With a pencil, number each test tube from one to twelve. C. For this experiment, you will add the measured amount of the first sample to the measured amount of the second sample into its respectively labeled test tube then observe if a reaction occurs. In your Data Table, record the samples added to each test tube, describe the reaction observed, if any, and whether or not a chemical reaction took place. D. Put on your safety glasses and let¡¦s begin: 1. Put the amount of 0.1M cobalt (II) chloride hexahydrate that fills the end of a spatula into a test tube. Then add 2mL of 95% ethanol. Tap the end of the test tube to mix the solution and record the pertinent data in section 1 of the Data Table. Discard the solution in the appropriate container as directed to you by your lab instructor. 2. Put 1mL of 0.1M cobalt (II) chloride hexahydrate dissolved in 95% ethanol into a test tube. Then add 1mL of deionized water. Tap the end of the test tube to mix the solution and record the pertinent data in section 2 of the Data Table. Discard the solution in the appropriate container as directed to you by your lab instructor. 3. Put a sample of zinc into a test tube.
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.
We then took 1ml of the 1% solution from test tube 1 using the glucose pipette and added it to test tube 2, we then used the H2O pipette and added 9ml of H2O into test tube 2 creating 10ml of 0.1% solution
For this experiment we are going to use concentrations, 0, 0.25, 0.50, 0.75 and 1.00 all measured in moles. To make sure these concentrations are accurate I will use a syringe to measure out the concentrations. I will use this table to help me.
To complete this lab several chemicals must be measured and transferred to test tubes. First 5.0 mL of 0.200 M Fe(NO3)3 must be diluted to a total volume of 50 mL in a flask. Next 0.0020 M SCN–. This solution is then added to 4 test tubes in 1 mm increments. Each test tube is then put in to
Planning Firstly here is a list of equipment I used. Boiling tubes Weighing scales Knife Paper towels 100% solution 0% solution (distilled water) measuring beakers potato chips Cork borer. We planned to start our experiment by doing some preliminary work. We planned to set up our experiment in the following way.
Use glassware as directed by your instructor. Place a test tube placed inside a beaker with ice water to collect the product from the apparatus. Obtain the 10mL round bottom flask from the apparatus. Obtain two graduated cylinders of 10mL. On one graduated cylinder measure 4mL (85% H3PO4) of Phosphoric Acid and pour into the 10mL round bottom flask. On the other graduated cylinder measure 3mL of Cyclohexanol and pour into the flask as well. With a pipet add 5 drops of Sulfuric Acid (H2SO4) into the flask. Attach the round bottom flask to the distillation apparatus. Place thermometer with rubber stopper on the apparatus to obtain the temperature Start with the water flow through the condenser. Turn on and heat the reaction until the product starts to distill. Distill and collect until thermometer temperature rises to 85˚C. Once there is no more product to collect obtain the test tube of product. Two layers should be formed, top layer of cyclohexane and bottom layer with water. Obtain a pipette and remove the bottom layer (water) if any. Add 10% (5mL) of Sodium Bicarbonate (NaHCO3) to nuclearize any acid in the solution. Mix well and remove once again the bottom layer of water with pipette. Add 5mL of water and mix well to wash the top layer. After the two layers form again, remove entirely the bottom layer of water and add a few pellets of Calcium Chloride. Obtain a 50mL or 100mL beaker and weigh.
The procedure is very short. First, I constructed the data table. I then massed one piece of Aluminum foil and record it in the data table. Next, pour 25.0 mL of 0.400 M Cu²+ solution and tear up the massed piece of foil. Drop the torn pieces in the solution and record the observations. Mass the other pieces of Aluminum foil, tear it up, and drop it in 25.0 mL of the 0.200 M Cu²+ solution. Record observations and clean up according to the teachers
By doing this experiment, I can know the physical and chemical properties of these samples. After I get my results about the physical and chemical properties of these samples, I can compare my results with the information given by the past student and identify the 5 unknown samples, finding out which sample is which substance. Hypothesis = ==
== § 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 = == = =
* Size of potatoes * Diameter of each potato tube * Time in sugar solution We need to make sure in both experiments the fair test lists are used and the procedures are carried out. This needs to be done otherwise my results will not be accurate and will look odd. Method: Firstly we got out all our equipment.
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.
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.
Ties and hair should be tucked out of the way, so they do not make contact with any of the chemicals. It would also be preferable to wear a scientific apron, however this is not essential. We should also try our best not to spill any chemicals, and we must not eat or drink in the lab while dealing with these harmful chemicals, as they can get on our hands. Fair Test To make this experiment a fair test, we need to make sure we do a number of things. In this experiment we are trying to find the rate of reaction using concentration as a factor, so there are a number of things we need to make sure we do to keep it a fair test.
Ultimately when conducting this experiment I need to look at how to determine chemical change and how to measure
tube. Add 6 mL of 0.1M HCl to the first test tube, then 0.1M KMnO4 and