Place it on the stand and begin heating it to the boiling point (100 degrees Celsius). 3. Measure the mass of the zinc to be tested. 4. Place the test tube, with the zinc in it, in the water and continue heating.
Measure and record the mass of the test tube and metal. 5. Place the test tube containing the metal into the beaker of water and continue heating (10 min). Leave the test tube in the boiling water bath while you complete steps 6 and 7. 6.
The term Cp is the specific heat of the material (at constant atmospheric pressure). Different materials have different specific heat values. The units of specific heat are : Joules/gram deg – C. In this lab we will find the specific heat value of Zinc and compare it to accepted values.This will do by heating a mass of Zinc up to the temperature of boiling water and placing the hot metal into a cup of cold water. The thermal energy that the zinc loses goes into heating up the water in the cup. By knowing the starting temperatures and the final temperature of the water and the zinc, the specific heat of Zinc may be easily obtained.
In the case of this experiment one of the reactions performed will have the same amount of heat released as the other two reactions combined. There are three reactions that take place in this experiment. They are as follows: · NaOH(s) à Na+(aq) + OH-(aq) · NaOH(s) + H+(aq) + Cl-(aq) à H2O(l) + Na+(aq) + Cl-(aq) · Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) à H2O(l) + Na+(aq) + Cl-(aq) It is important to be aware of these reactions in this experiment for one reason; knowing the reactions will allow one to combine equations for two reactions to obtain the equation for the third reaction. There are also several math related concepts that one should be aware of in this experiment. First, when determining the mass of 100 mL solution, it is necessary to assume that the density of all the solutions is 1.00 g/mL.
Gravimetric Determination of Sulfate Purpose The purpose of this lab is to determine the percentage of sulfate in the hydrate by precipitating the sulfate as barium sulfate. Materials Filler paper Sodium sulfate Graduated cylinder Bunsen burner Watch glass Beakers (250 mL, 400 mL) Rubber bulb Graduated pipette Beaker tongs Funnel Filter Paper Sodium Sulfate Drying oven Wash bottle Stirring rod Silver nitrate Hydrochloric acid Distilled water Small test tube Procedures First, .4861 grams of sodium sulfate was placed into a clean 400mL beaker. Exactly 200mL of water and 1mL of HCl was added to the same beaker. A watch glass was placed on the beaker and the solution was heated using the Bunsen burner to a gentle boil. The watch glass was removed with the beaker tongs.
Laboratory 2/3 will follow the rate at which aragonite transforms to calcite. The effect of magnesium will be determined throughout the reaction in which aragonite turns to calcite. From a comprehensive analysis of the data collected, it will be determined if magnesium does, in fact, act as an inhibitor throughout this process. 2.0 Methods 1M CaCl2 and 0.1M Na2CO3 were prepared and measured by the teaching assistants prior to the lab. The premeasured solutions were then placed on hotplates bringing them up to their desired temperature.
Now right-click on the flask, and select Heating Mantel from Distillation Equipment then, Right-click on the flask, and select Distillation Head from Distillation Equipment last, Right-click on the flask, and select Condenser from Distillation Equipment. Now, right-click on the flask, and select Distillation Take-off from Distillation Equipment. From the Equipment menu, select the 100 mL Graduated Cylinder. Place it under the end of the distillation take-off. The graduated cylinder will collect the distillate.
Experimental Procedure: 250 mL of the copper solution was made by creating 100 mL of the solution, reacting CuO with HNO3, and then diluting to the mark of 250 mL. Using this stock solution, different concentrations were made and placed in the sprectrometer for observation. The absorbances and transmittances were recorded for use when identifying the amount of the color-absorbing copper ions later. A graph was plotted of Absorbance v. Molar Concentration easily see the results of the experiment. Pre-Lab Questions: 1.
Part 1 of The Redox Arena Objective: In this experiment, we had to conduct research on zinc, iodide, and acidified water. What my partner and I did was we mixed the aforementioned elements with acidified water to see what would happen. We took notes on the physical traits of each, and then we compared out qualitative results with the three samples we had. Materials & Observations: * electronic balance * Bunsen burner * Parafilm * Spatula * Boiling tube * Corks * large beaker * Stirring rod * large test tube * test tube rack * small graduated cylinder * pipets * grease pencil * Ziploc bag * Boiling chips- off white, small pebble like pieces * Desiccant- white small rocks, chalky * Acidified water- clear liquid * Sodium thiosulfate- clear liquid * Granular zinc- gray, small, mineral like * Iodine crystals- dark grey, shiny solid * Zinc ion- grey, irregular shaped * Solid zinc iodide- white solid * Mineral oil- colorless solution The Mass table was as followed: Chemicals | Amount | Granular Zinc | 2.01 grams | Iodine Crystals | 2.01 grams | Acidified Water | 5.0 mL | Procedure: 1. Obtain a boiling tube, a large test tube and a small test tube.
C121 Elementary Chemistry Lab I “Building a Better Water Filtration System: An Investigation of the Properties, Changes, and Composition of Matter” Ian McGrath September 30, 2012 Period 1 “Building a Better Water Filtration System: An Investigation of the Properties, Changes, and Composition of Matter” Objective – Make a filtration system to filter the polluted water Reference – Mr.Harnish Procedure – 1. Put on safety goggles and lab apron 2. Make a filtration system using the PVC pipe 3. Cover bottom with cheesecloth and tie it with a rubber band 4. Get 200 mL sample of polluted water and place into 250 beaker 5.