1. Read MSDS sheets and record any precautions in the data table. 2. Observe and record the colour of every substance. 3. Fill up the 50 milliliter beakers all the way up with deionized water. After, use your scopula to scoop out a small portion of one substance and put in into your beaker. Then put your hot plate onto medium temperature and rest the mixture onto the plate. Using the scopula, take a small amount of the substance and add it to the spot plate. Add deionized water to the section with the substance. Stir to see if the substance dissolves or not. Record your observations. 5. Observe and see if the substance dissolves in the solution. Record your observations. 6. Pour the solution down out of your beaker and rinse the beaker that
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.
the large beaker pour in some more hot water or if it is too hot pour
...row.Place a coffee filter in a funnel.Place the funnel in the top of the second glass canning jar.Slowly pour the solution over the filter,but not too much.Let it collect in the jar.Looking at the coffee filter,what do you see?Record your observations in the “Observations after separation” section.Carefully scrape off any particles on the filter with a spoon and put them in the first jar.
A team was sent to the chemical manufacturing division of a small chemical company to help the technicians with experiments. Since the notes written by the technicians were inaccurate and unfinished, all of the experiments they had preformed needed to redone and documented correctly. The head of the company gave the new team the task of trying to figure out why some chemical reactions caused the reaction vessel to get cold and others caused the vessel to get hot. The group constructed ¡°an apparatus to measure the quantity of thermal energy gained or lost during the chemical reactions¡± (Bellama, 193). This device was called a calorimeter. A series of different reactions were conducted using two different calorimeters. First, hot and cold water tests were preformed. Based on these results the scientists calculated the heat capacities of the calorimeter. The density and specific heat of pure water were used for these calculations. The other tests that were redone and recalculated were: salts in water, precipitation reactions, and acid base reactions. Then the question of whether the solution absorbed or gave off heat can be answered. Also, whether or not the concentration of an acid base reaction made a difference in the heat absorbed or lost can then be resolved. The goal is to determine if the reactions gave off heat or became cold. The factors that affect heat energy changes were identified (Cooper, 103).
1Fill one of the glass with very hot water. Add a drop of red food
The porpoise of these is to determine the Specific Heat. Also known as Heat Capacity, the specific heat is the amount of the Heat Per Unit mass required to raise the temperature by one degree Celsius. The relationship between heat and temperature changed is usually expected in the form shown. The relationship does not apply if a phase change is encountered because the heat added or removed during a phase change does not change the temperature.
After the water, has been boiling for 10 minutes, and the temperature inside the test tube has been stable for 5 minutes, record the temperature and remove the thermometer.
Then add growth media until the sample is submerged beneath the 2-3 ml of liquid, cap the tube and invert several times to mix thoroughly, incubate the tube while shaking vigorously in a shaking incubator at 250 rpm for a couple hours, then allow the sample to sit.
The objective of the lab is to determine the heat of the reaction between magnesium and hydrochloric acid in the calorimeter. To determine the enthalpy change of the chemical reaction, a calorimeter was placed onto the workbench. A balance was place on the workbench. The calorimeter was placed onto the balance and weighed to be 18.600 grams. A thermometer was attached to the calorimeter. The initial temperature recorded is 21.5 C. 50 mL of 1M of Hydrochloric Acid was placed into the calorimeter. 0.150 grams of magnesium was added into the calorimeter. A chemical reaction had occurred and the observed temperature was 34.5 C. The calorimeter was placed onto the electronic scale and was measured to be 68.738 grams. The used calorimeter were
7.) After you have heated them to the right temperatures, pour the excess water into a dry evaporating dish. ( Be sure not to get any of the substance in your solution. )
In a 100ml beaker place 50mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved.
Fill a glass or beaker with with roughly 120ml of water, add enough ice to adjust the level to 200ml. Stir the ice water and wait until ice is dissolved, make sure water is roughly 200ml, if not add more
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.
(iii) Transfer the sample to pre-weighed dish and evaporate to dryness on a drying oven at low temperature to approximately 2ºC below boiling to prevent splattering.
Measure out 12ml of distilled water using a 10ml measuring cylinder and pour into a 25ml beaker.