Dip a cotton swab in each solution and hold to a flame. Observe the color of the flame with the soaked cotton swab. Use the 7 known compounds to determine the unknown ion solution. Data Table: Metallic Ion | Flame Color | Sodium Na+ | orange | Strontium Sr2+ | bright red | Potassium K+ | pinkish/purple | Lead Pb2+ | Did not come with our lab kit | Barium Ba2+ | yellow/white | Copper Cu2+ | green | Lithium Li+ | pink/red bright | Calcium Ca2+ | pink | Unknown (Sr2+) | orange/red | Observations: When passing the cotton swabs soaked in different ions through a flame many colors were noticed. For some of them there was a cracking sound.
The color of KCl is present in a color that is lavande. A mixture of violet and blue. When NaCl is burn the energy is released in packages of light which its color is yellow-orange. When NaCl is burn the energy is released in packages of light which its color is yellow-orange. OBSERVATIONS: Data Table 1: Reactions of elements after been burned.
Allow the mixture to cool for a few minutes then filter it, using either gravity or vacuum filtration. (We shall be using vacuum filtration.) Wash the residue in the funnel once with a little water and collect all the filtrate. 4. Pour all the filtrate and washings into a 250cm3 volumetric flask.
4. Any hanging drop was removed from the jet, and the sodium hydroxide was then drawn up using the pipette, to above the graduation mark and allowed to run into the sink. This process was the rinsing of the pipette. 5. Sodium hydroxide was again drawn up using the pipette, to above the graduation mark, where the meniscus was allowed to fall until the bottom of it was rested on the graduation mark when viewed at eye level.
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.
Stirring carefully and observe the color of the hydrate until it changes to a consistent white color, then the Copper(II) Sulfate is dehydrated. 6. Turn off the burner, and wait to cool down the material. 7. Carefully determine the mass of the Copper(II) Sulfate, crucible, and lid.
First obtain 2 crucibles and lids. Label them #1 and #2. Make sure to clean the crucibles thoroughly. Now for part 1; weigh the crucible without the hydrate before heating. Then weigh the crucible without the hydrate after heating.
6- Place only the edge of the Q-tip at the top the Flame. 7- Remove it when you see the of light being given off to avoid burning the Q-tip. 8- Clean up procedure: Discard used Q-tips to the bin, cover back compounds and put them up in a safe place, pour away distilled water in the sink, disconnect the Bunsen burner and clean it if stained,clean the lab test surroundings with paper towel to ensure no stain is left, wash your hands remove your goggles only when all equipments have been placed in safe places. Compound | Flame Colour Observation | 1 LiNO3
Clean the nichrome wire by dipping it into the acid and heating the loop to get rid of any excess chemicals. Dip the wire into one of the sample solutions and place into the hottest part of the flame. Repeat the dip into the salt solution if necessary to see the flame test colour. Write the colour of each metal salt when it is put into the flame into a results table. Repeat this procedure with the other known solutions to record the
The watch glass was removed with the beaker tongs. Using a rubber bulb and a stirring rod to stir the solution continuously, 15.00mL of .25M BaCl2 solution was added to the solution in the beaker. The watch glass is replaced and the solution is keep hot but not boiling for 15 minutes. The precipitate was allowed to settle. When the liquid above the precipitate was clear, the solution was tested for completeness of precipitation when a few drops of BaCl2 solution were added from a pipette.