Specific Heat of a Metal Michael Diaz Ms. Zhort Performed: October 3, 2013 Due: October 24, 2013 Period: 1 Lab Partner: Rocco & Asha Objective: This lab was meant to teach us how to find the specific heat of a metal sample. Materials: * Specific heat set * Balance * Thermometer * Tap Water * Hot plate * Polystyrene cup and a lid * Stirring rod * 250 mL beaker * String (about 15 cm) Procedure: 1. Fill a 250 mL beaker approximately half full of water. Place the beaker of water on a hot plate. Begin heating the water to the boiling point.
While the water is heating, remove the foil from Erlenmeyer flask and place about 2 mL of unknown liquid in the flask; then replace the foil and rubber band. 6. After the water has been brought to a boil, record its temperature. 7. Insert the Erlenmeyer flask into the boiling water.
Gently stir the pellets until the acid is dissolved by shaking the the apparatus. Lift the calorimeter lid and wash out its contents and the thermometer. Repeat this experiment using 50.0 mL of 1.0M acetic acid. Repeat experiment using 25.0 mL of each 2.0M sodium hydroxide and 2.0M acetic acid. Data Table(s): Reaction equation Mass of solid NaOH Initial Temp.
A melting point will be ran on the aspirin when completely dry. A capillary tube containing the dry aspirin will be placed into the melting-point apparatus. This process is to determine the melting point range of aspirin. First, a hot water bath was created with a 400. mL beaker on a hot plate. The temperature was raised to 70 degrees Celsius and 4.419 g of salicylic acid was measured out on a balance and transferred into a 125. mL Erlenmeyer flask.
7. Cover the lid and place the thermometer inside to measure the temperature change. Data Collection: Trial #1: Mass of the unknown object Initial temperature T1 (◦C) ± 0.5 Final temperature T2 (◦C) ± 0.5 Calorimeter 200mL of H2O 20 32 Beaker 200mL of H2O 20 86 Trial #2: Mass of the unknown object Initial temperature T1 (◦C) ± 0.5 Final temperature T2 (◦C) ± 0.5 Calorimeter 200mL of H2O 20 29 Beaker 200mL of H2O 20 87 Data Processing: We know that the heat lost by the water is equal to the heat gained by the unknown object. Therefore mwcw∆Tw = mobjectcobject∆Tobject is true. Trial #1: mw = 200g cw = 4.18 kJ/kgK, ∆Tw = 97 – 20 = 77◦C mobject = 21.7g cobject = ?
1ml of concentrated H2SO4 was then added to the tube and the solution was continuously stirred to dissolve all the triphenylmethanol. Using a Pasteur pipette, the sulfuric acid solution was then transferred to 2ml of ice cold methanol. Crystallization was induced by scratching the tube with a glass rod. The crystals were collected by vacuum filtration on a Hirsch funnel. After filtration, the crystals collected were washed thoroughly with water and then dried with filter paper.
Equipment List * Boiling Tube * 10 cm3 1mol dm-3 Hydrochloric Acid (HCL) * 15 cm3 1mol dm-3 Sodium Hydroxide (NaOH) * pH and Temperature Probes * Data Logger * Measuring Cylinder ‘ * Boiling Tube * Teat Pipette Method * Add 10ml of Hydrochloric acid, measured in a measuring cylinder, into a boiling tube. * Into a data logger, plug in both pH and temperature probes and switch on data logger. * Put in both the probes and measure both the temperature and pH before adding any other substances. * Add 1cm3 of Sodium Hydroxide, measured in a measuring cylinder, to the Hydrochloric acid, and
The mixture was decanted again in to the same beaker. Next, we added boiling chips to the liquid and evaporated the solvent over the hot plates under the hood. After the solvent was evaporated and the flask was cooled, we used a spatula to remove a small amount of the crude product and took its melting point. We determined the melting point range of the sample to be 43.0-46.0 degrees Celcius.The crude product was yellow colored when it was warm and orange in color when cooled and sticky. We then recrystallized our sample using 5 ml of warm acetone that was heated on a hot plate under a hood.
How I did this was to note down the colour of the flame from each different metal salt solutions. Method: To do this experiment you will need a Bunsen burner, nichrome wire loop, hydrochloric acid 2M, salt solutions and water samples. First of you will need to clean your nichrome wire loop by dipping it into the beaker of hydrochloric acid 2M and then placing the wire into the flame until no colour is visible. Next you will need to get your 7 different metal salt solutions which are: Lithium, Sodium, Potassium, Copper, Calcium, Barium and Strontium, then one by one dip the nichrome wire loop into the hydrochloric acid and into your first metal salt solution which would be Lithium and then place the nichrome wire loop with the metal salt solution in the edge of the flame, Then finally when a colour shows in the flame note it down along with the name of the metal salt solution you are testing. Repeat this with the following metal salt solutions: Sodium, Potassium, Copper, Calcium, Barium and Strontium.