Isolate area for 100 meters in all directions. Use a chemical extinguisher to put out any fires. first aide- move victim to fresh air, administer o2, remove all contaminated clothing, if in contact with skin and eyes flush for 20min. Immediately cool burned areas with warm water and don't remove any clothing stuck to the skin. thaw any frosted parts with lukewarm water if contacted by a liquefied
Measure 0.10 g of copper powder within 0.098 to .102 g 2. Put the copper into a 140 mL beaker and move the beaker to the fume hood. 3. Slowly add 2mL of concentrated nitric acid (8M) to the copper and swirl the beaker so all the copper can react with the nitric acid. 4.
Obtain an Erlenmeyer flask that has a vacuum opening and attach the vacuum tube to it 8. Insert funnel and rinse the funnel with distilled water 9. Turn vacuum on and pour the pink solution into the Erlenmeyer flask, the precipitate should stay on top of the filter 10. Rinse the beaker out until all residue is gone 11. Try to rinse the precipitate in the funnel until the pink color is gone 12.
The aspirator was turned to medium high, and then the copper was poured onto wetted filter paper. Using distilled water to remove all copper from the beaker. Once completely on filter paper 6mL of acetone was added to the copper to help dry it out. The filter paper was then removed and set down to dry completely. Once dry the filter paper was weighed with the copper on it and subtracted from the original weight to see the amount of copper left after
10-29-10 Analysis of Alum Purpose: To determine if the sample crystals are really aluminum potassium sulfate or alum. Materials: alum, beaker, hot plate, thermometer, thermometer clamp, mortar, pestle, capillary tubes, small rubber bands, stirring rob, goggles. Procedure: Determine the melting point: 1. Pulverize with pestle about 2.00 grams of alum. 2.
When air (oxygen) is in contact with combustible material (fuel) at a high enough temperature, a fire begins. Water, the most common extinguishing agent used in urban areas by firefighters, reduces the temperature of fuel below it's ignition point. Consider that a bucket of water will put out a small campfire by cooling the burning fuel (wood) below the point of combustion. By the way, there is a chemistry term for the point at which a chemical reaction begins: activation energy. (As you can guess, different fuels begin burning at different temperatures.)
Allow the splint to burn until the color fades. Don’t let any solids to fall into the burner. -Soak the wooden splint in the “rinse water” to put it out completely; move it to trash. -Record observations on flame color produced by the metallic salt in the Data Table. -Repeat above steps (middle section) for all metallic salts (five total).
I then took the initial temperature of the water. I grabbed my marshmallow and weighed it then weighed the fork. After recording the weight I lit it on fire with the lighter. Once it had a steady burn I placed it under the beaker and stirred the water with the thermometer. Once it stopped burning, I took the final temperature of the water.
Using the utility clamp, clamp the thermometer, attach the paper lid to the probe then move the probe close to the bottom but not touching the magnetic stirrer. Start the Logger Pro program on the computer. Open the file “13 Enthalpy” from the Advanced Chemistry with Vernier folder. Measure 50.0 mL of 2.0 M Hydrochloric acid, HCl, solution and pour into the styrofoam cup, make sure that the temperature probe is touching the solution. Measure 50.0 mL of 2.0 M Sodium Hydroxide, NaOH, solution but DO NOT ADD YET.