Cation Flame Test Lab Report

We then proceeded in testing for excess Ca2+ by adding two drops of .5 M K2C2O4 to test tube two and attentively observed to see if a precipitate formed, which it did. This meant that Ca2+ was in excess and C2O42- was the limiting reactant in the original salt mixture. We then cleaned up. Upon returning to our next class, we took the filter paper, with the precipitate on it, and took its mass.

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

Solub. Or Reaction w/ hot H20: no change observed from the cool water and is soluble

Examine a piece of nichrome wire. On the data sheet, record the color and the luster of the metal. Use a forceps to hold the wire in the flame of your burner for about two minutes (recall where the hottest part of the flame is located). Describe the appearance of the wire while held in the hottest part of the flame. Allow the wire to cool and reexamine it. From your observations, determine if there was a physical or a chemical change. Give specific reasons for your conclusions. Save the nichrome wire for step #2.

The problem that was trying to be solved in this study deals with analyzing unknown solutions. In this particular case, a chemical company has several unknown solutions and to correctly dispose of them they need to know their properties. To figure out the properties several qualitative tests were performed throughout the study (Cooper 2012).

Solutions of 6M H2SO4, 6M NH3, 6M HCl, 6M NaOH, and 1.0 M of NaCl, 1M Fe(NO3)3, 1M NiSO4, 1M AgNO3, 1M KSCN, 1M Ba(NO3)2, and 1M Cu(NO3)2 were given in separate test tubes. The color of possible precipitates, ions, acid-base behaviour, odor and solubility rules were conducted and were reported in Table 1. The key information about a mixture of two solutions was

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,

To study the nature of ionic reactions, write balanced equations, and write net ionic equations for precipitation reactions.

For example, silver nitrate formed a white precipitate when it was tested with ammonium chloride. In contrast, unknown 3 did not formed any precipitate with ammonium chloride. Ammonium chloride change the color of unknown 3 to a light green while the solution of silver nitrate and ammonium chloride was cloudy white solution. Likewise, the metal in unknown 3 could have been Calcium neither. Data and observation shows that calcium nitrate whether formed a white precipitate or did not react at all while unknown 3 formed an orange precipitate. Therefore, silver and calcium are not the two metal present in unknown

In this lab we performed four test. Using these test we discovered how the chemicals compounds Citric Acid, Calcium Chloride, Sucrose, Potassium Iodine, Phenyl Salicylate , and Sodium Chloride reacted to heat and many solutions. We also noticed that Phenyl salicylate was the least reactive out of all chemical compounds. Using the information discovered from the lab we were able to separate the chemical compounds into two groups. In group one were the chemical compounds Calcium chloride, Citric acid, Potassium iodide, Sodium chloride, and Sucrose these chemical compounds reacted to three of the four test. Group two was just Phenyl salicylate which reacted to only one of the four test. We also were able to state that group one was a covalent compound group and, group two was an ionic compound

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

This information would be used in Part III to determine an unknown mixture with the results that were found in Part I. A singular drop of Pb(NO3)2 , Fe(NO3)3 , Ni(NO3)2 , AgNO3 , Ba(NO3)2 were added to the reagents: K2CrO4 , KSCN, NH4OH, DMG, HCl, H2SO4 inside of the glass spot plate. If a precipitate formed than the combination resulted in a change of color or appearance (results to these reactions are found in table 1.1). Part II included using the same procedure as done in Part III except this sample contained 1 mL of all five metal ions. This was meant to be a practice round to understand the different steps and procedures. Unfortunately, due to time concerns this trial was cut short at step 3.

The purpose of this lab is to determine the chemical and physical properties of an unknown substance. Then, through the use and practice of some basic techniques used for analyzing compounds, find a compound that shares similar traits. Some of these basic techniques that were performed include: using a magnifying glass to determine the physical characteristics, solubility, conductivity (solid state/aqueous solution), pH test of the aqueous solution, reactivity test with Lead Nitrate, Hydrochloric Acid, and Sodium Hydroxide, a flame test, and melting point based on the time it took to reach it within 20 seconds. With these tests one can narrow down unknowns using the results, and then finally run confirmatory tests to solidify the findings.

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

Two samples of unknown #8 were taken and weighed at 0.4004g (Sample 1) and 0.3985g (Sample 2). The two samples were placed into separate 400 mL beakers along with 200 mL of DI water containing 4 mL of 6M HCl. Two samples of the BaCl2.2H2O weighing 1.51g each were placed into separate 250 mL beakers and dissolved using 100 mL of DI water. 95 mL of each of the BaCl2.2H2O solutions were added to the earlier mentioned 400 mL beakers containing the unknown #8 solutions, leaving roughly 5 mL to later test completeness of precipitation of the sulfate ion. The newly added mixtures were heated for 3 minutes and then were allowed to cool and settle for 10 minutes. The remaining 5 mL of BaCl2.2H2O solution was added to their respective unknown solutions to ensure precipitation completeness of sulfate ions. Upon completeness, the two solutions were heated for 90 minutes at near boiling temperatures. After the 90 minutes, the solutions were removed from the heat, cooled, covered with parafilm and stored until the following week.