Flame Test Lab Report Essay

The purpose of this experiment is to identify three unknown solutions through the flame test. To attain this purpose, seven known solutions were first tested for their colors as seen in Table 1. To avoid potential contamination, droplets of solution were placed in a watch glass. The nichrome wire was heated with the flame generated by the Bunsen burner. Then, the wire was dipped into solution on the watch glass.

Pour 50 mL of distilled water into a 100 mL beaker, and then add the unknown substance into it. Mix thoroughly to create the aqueous solution. Now fill a new cuvette with this new solution and place into the SpectroVis Plus device; after wiping the outside with a Kimwipe as usual. Be sure to take note of the absorbance when wavelength is at its maximum. Afterwards, Be sure to take all solutions containing Iron(III) and pour them into the container specified for hazardous wastes. ​

Eleven mystery test tubes labeled from K-1 to K-11 contained: 6M H2SO4, 6M NH3, 6M HCl, 6M NaOH, 1M NaCl, 1M Fe(NO3)3, 1M NiSO4, 1M AgNO3, 1M KSCN, 1M Ba(NO3)2, 1M Cu(NO3)2 respectively. The contents of the test tubes were determined by chemical experiments. Solution K-1 contained NiSO4 because when solution K-9, ammonia which was identified by its pungent odor, was added, an inky dark blue color was made. Iron (Fe (NO3)3) was determined to be in test tube K-2. KSCN was found in test tube K-11 since Fe (NO3)3 and KSCN makes a bloody color when mixed together. Flame tests were conducted in which K-8

2. If the mineral is non-metallic, decide if it is light or dark in color.

We repeated this for a total of 6 known substances and 3 unknown substances. We also made a table for each element showing the color of the flame that we saw,

The flame test had a variety of results. Most of the known compounds did not match our unknown except for Ca(NO3)2. Both Ca(NO3)2 and the unknown compound had a deep red/orange color flame. While Ca(NO3)2 had the closest results two other compounds had slightly different results but not different enough to rule them out. Those other two compounds were CaCl2 with a yellow/ orange color and CaCO3 with a reddish color.

4. Why does the flame color change back to orange, after the metallic solution has been turned completely into a gas

To perform the experiment, you need 2 ml of water, then contain 15 ml of 3m HCL, 6m HNO3, 6M NaOH, then 15 ml of unknown solution each one labeled on a test tube. A flame test will be conducted to determine ions. You will need a spot plate, Bunsen burner, flame-test wire, dropper bottles of 0.1 M NaCl, 0.1 M KCL, 0.1 M CaCl2. Obtain a spot plate. Place 5 to 8 drops of 0.1 M solutions of each of the following solutions into separate indentations: KCL, CaCl2, NaCl, unknown solution. To clean the flame-test wire dip the loop at the end

The indicators of the chemicals changes that has happened were, heat was produced (when the blue flame occured because of methane and oxygen gas heated the watch glass) in reaction 1, the bottom of the watch glass became black (changed colour and a precipitate was formed) due to the same procedure but less oxygen for reaction 2, and the colour changed for the foil and bubbles/gases were produced for reaction 3. Moreover, in reaction 4, the colour of the copper also changed and the smell was like smoke. In reaction 5, the colour of the solution changed continuously as mentioned in the observations, with bubbles, gases (oxygen), and heat were produced. And lastly in reaction 6, hydrogen gas were produced because of the burning splint test, indicating that a gas was produced. Temperature change occurred in some of these reactions (e.g., reaction 1, reaction 5, etc.), making it one of the indicators of a chemical change as well.

In this project we examined three explanations that talk about (a) candle(s) in a jar and their investigation reasoning to why the labs they did were concluding in such a way. The first explanation resulted that the candle inside the jar took up all the oxygen molecules inside the flask which then lowers the pressure inside and the higher pressure outside the flask is what causes the water to rise up. The second explanation resulted in that the air pressure increases inside the jar because of the heat from the candle, which causes air to come out of the jar and once the candle cools down the pressure decreases and the pressure outside the jar increases which results in pushing the air in and making the water rise up. The third explanation resulted in oxygen inside the flask becoming carbon dioxide which then dissolves in water causing the air pressure to decrease under the glass and the higher pressure outside the flask pushed the water up the flask. I believe that explanation number three is right because the flame causes carbon dioxide to be created and that

Objective: The objective of this experiment was to discover the specific heat of an unknown metal. By heating a metal then placing it in a calorimeter and taking the temperature of the solution as the heat transfer from the metal to the solution. This is done using a calorimeter, thermometer, 2 200mm test tube, an unknown metal, hot plate, 2 50ml graduated cylinders, sodium hydroxide, and hydrochloric acid. The techniques that are used in this experiment is cleaning glassware, disposing of chemicals, measuring mass, transferring solids, transferring liquids and solutions, heating liquids and solutions, and measuring the volume of solutions by examining the meniscus. Introduction: Chemical reactions always exerts some form of thermal energy, that energy then applies changes to its reactants, this is called Calorimetry which is the analysis of temperature change or heat change within a chemical reaction.

Experiments were conducted to test the heat along with different variables of certain chemicals when burned in a flame test. My study focused on 7 chemicals: Lithium Chloride, Strontium Chloride, Copper 2 Nitrate, Sodium Chloride, Borax, Copper 2 Sulfate, and Potassium Chloride. The hypothesis stated that I believe Sodium Borate, or Borax will burn the hottest. The station was set up for chemical testing, and each chemical was prepped and the nichrome wire was cleansed.

The heat of combustion tables were calculated assuming complete combustion occurred. It is known that the experiment did not achieve complete combustion due to the lab conditions, percentage error and other experimental flaws. If complete combustion occurred there would have been no carbon monoxide released as soot and the flame would appear more blue. The flame in the experiment was orange. Other factors such as wind and insulation affected the

The main objective of this experiment is to carry out qualitative analysis to identify metal cations in unknown solution 1.

The cations in both the known and unknown samples were identified by using qualitative analysis, of which were determined to be acidic, basic, or neutral by using litmus paper. Acid-base reactions, oxidation-reduction reactions, and the formation of complex ions are often used in a systematic way for either separating ions or for determining the presence of specific ions. When white precipitate formed after adding hydroxide, aluminum ion was determined to be present in the solution. However, nickel was determined to test positive when the solution changed to a hot pink color after adding a few drops of dimethylglyoxime reagent and iron was present when the solution was a reddish brown color when sodium hydroxide was added to the mixture at the very beginning of the experiment. Qualitative analysis determines that ions will undergo specific chemical reactions with certain reagents to yield observable products to detect the presence of specific ions in an aqueous solution where precipitation reactions play a major role. The qualitative analysis of ions in a mixture must add reagents that exploit the more general properties of ions to separate major groups of ions, separate major groups into subgroups with reactions that will distinguish less general properties, and add reagents that will specifically confirm the presence of individual