Flame Test Lab Report Discussion

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.

The beaker’s role in the experiment is very important, because without it the experiment wouldn’t work. During the experiment, the beaker was playing two roles, and the first one is that the beaker was placed over a fire on the candle, so anything released by the fire would be kept inside the beaker. The fire

Submitted by: Blossom Okpali Sumitted to: Mrs. Chui Course Code: SNC 1D Group members: Joy, Paulina and Christina Date assigned: March 27 2018 Due Date: April 6th 2018 Introdution: The flame test is used to help miners, geologists, and chemists identify the presence of chemical elements. They can be used to distnguish unknown metallic and metalloid ions, The heat from the flame excites the electrons of the metals ions, causing them to emit light. Every element has an emission that can be used to differentiate between one element and another.

In reference to the analysis of anions, Table 1 shows that a precipitate was formed when our unknown was combined with HNO3 and AgNO3, thus indicating the presence of a chloride ion. Because our unknown did not form a precipitate due to HCl and BaCl2, separate, effervesce, or smell, we concluded that neither sulfate, nitrate, carbonate nor

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

The objectives for the Limiting Reactant Lab was to determine out of the equation Ba〖Cl〗_(2 (aq))+ 〖Na〗_2 〖SO〗_(4 (aq))→ 〖BaSO〗_(4 (s) ) +2 〖NaCl〗_((aq)) which compound is the limiting reactant from choosing either A or B for the experiment. The purpose for part one is about 〖Na〗_2 〖SO〗_(4 (aq)) and Ba〖Cl〗_(2 (aq))*2H_2 O, when adding water and resulting in 〖BaSO〗_(4 (s) ) is allowed to precipitate. From the two values the percent yield can be calculated. The purpose for part two is the formation of barium sulfate.

This did not allow for all for the flames energy to be concentrated on one spot at the bottom of the beaker. This error would have decreased the precision and accuracy of the data gathered form the experiment. This chance of this error could be removed it the experiment was to take place somewhere were there would be not motion of the air to change the position of the flame (e.g. in a bomb calorimeter). 2. Variance in length and width of burner wicks.

In the lab, Bunsen Burner operation, we were given 6 known substances (Calcium Chloride, Copper Chloride, Lithium Chloride, Potassium Chloride, Sodium Chloride, and Strontium Chloride) and 4 unknown substances. The goal of this lab was to match 4 of the known substances to the 4 unknown substances. Scientists are able to do this because when the wooden splint is inserted into the hottest part of the flame the electrons entered an excited state and release energy in the form of visible light. The light emitted is unique for every metal ion because every ion has a distinct electron configuration. Scientists are then able to identify what substance was burned from the color of the flame.

Purpose: To accomplish this experiment, firstly will be analyzed a solution that contains six known cations and then, will be analyzed an unknown solution with the purpose of discovering the cations present on it. For this experiment will be conducted a qualitative analysis on the solution to identify the substances presents on the solution. In addition, this experiment will endow ones with a different perception about the nature of ions. Chemicals and Materials Required: Materials: 8 test tubes (12 × 75 mm), stirring rods, test tube holder, centrifuge, test tube rack, spatula, hot Plate, red Litmus paper, 400 mL beaker, blue Litmus paper, 100 mL beaker, Capillary pipet, and 250 mL beaker.

The experiment and the purpose of the experiment consisted of comparing known and unknown compounds based on established standards of flame color and solid compound characteristics. By observing the colors of the salts, we were able to conduct a flame test and identify it. My hypothesis was that by comparing the flame colors of metal ions to known standards, the identity of the salt compound could be determined. Ultimately, our hypothesis was proven right, and we correctly identified the known and unknown compounds. The justification for the hypothesis is because according the Bohr’s atomic model, electrons are found in energy levels outside of the nucleus.

RESULTS & DISCUSSION The purpose of this lab was to identify two different cations in an unknown solution by using qualitative analysis. The two methods of qualitative analysis explored in this lab were precipitation reactions and cation flame tests. If this lab were to be performed again, it would be beneficial to switch the order of Step 13 and Step 14 to confirm or deny the presence of calcium first before confirming/denying the presence of barium due to the possibility of a false positive from the barium.

The purpose of this experiment was to use qualitative analysis—manipulating the chemical and physical properties of a certain species—to determine the identities of two cations in an unknown solution. In Part A, the goal was to determine whether the solution—composed of metal nitrate salts—contained lead (Pb2+) or silver (Ag+). Afterwards, in Part B, the goal was to determine whether the solution contained barium (Ba2+) or calcium (Ca2+). Finally, in Part C the goal was to identify cations in specific solutions though the cation flame test.

During this lab we investigated the different flame colours produced by different compounds when electrons are excited by heating method, by doing this we were managed to identify two unknown compounds by comparing their flame colour to known ones. In this lab we used nichrome wire to pick up different compounds to burn in Bunsen burner to examine the different flame color, after each compounds, we cleaned the nichrome wire by rising it in hydrochloric acid and burning it until no colour other than the flame's natural color was observed. By burning the compounds we excited the electrons to undergo transition, when they fall back to ground state, they emit light, and each element has different energy, which means they produce different colour of light. By looking at the results and observation, we saw that the flame color of sodium nitrate and sodium chloride was same, or almost identical. We figured out that it was the cation of the compound, which was responsible for the different colour we see, and not the anions in this experiment. Also by doing this we figured out the unknowns by comparing the flame color, the unknowns had the same colour as lithium nitrate and calcium nitrate, so I will assume the unknowns are lithium nitrate and calcium nitrate, but we

The observation of chemical behaviours under specific conditions allowed for the use of process of elimination. Given the observations found in the materials and methods section and the data found in the lab manual1 it was found that the anion was not acetate or carbonate, but rather a halide, specifically Br due to the brown-yellow hue of the organic layer. The observations for the cation test along with the data from the lab manual1 showed that the unknown was from group II. Since the flame test showed no observable difference this allowed for the conclusion that the cation was Mg2+.

What did you observe when the popsicle sticks were placed into the bunsen burner flame?