Alkaline Earth Cation Lab

6-3: This process is used by cells to manufacture _biochemical energy from nutrients into adenosine triphosphate (ATP), and then release waste products__

In experiment A the results from the precipitation of CaC2O4 H2O from the salt mixture were obtained by weighing the items listed on Table 1 on a scale.

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

* By using the dropper and measuring cylinder, 7 ml sodium carbonate solution was added to the test tube

In doing so, the identity of the unknown solutions was determined through comparing the colors of the unknown to that of the known, which were dependent on the varying energy transitions the electrons went through. Therefore, the purpose of the experiment was successfully achieved. Since LiNO3 and Sr(NO3)2 were red/red orange in color, it was determined that lithium ions and strontium ions have the least amount of energy due to the fact that red has the longest wavelength in the spectrum, and colors with longer wavelengths have lower energies. The energy of each the other metallic ions increased in accordance with the energy of the wavelength emitted from that color based on the color spectrum. Potassium had the highest energy emitted, since violet is at the opposite end of the spectrum and has the shortest wavelength and highest

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).

Based the data collected, the identity of the unknown #42 is lithium chloride. Because the unknown compound produced a bright red pinkish flame, shown in Table 1, the possible cations based on the CRC Handbook were lithium or strontium 1.The known 1M lithium chloride also produced the same colored flame as the unknown, suggesting that the unknown compound has lithium. Since lithium produces no precipitate with the compounds in Table 2 and strontium produces a precipitate with the same compounds, the observations in Table 2 indicate that the unknown’s cation is lithium 4. Using the solubility table, process of elimination, and the results in Table 3 the possible anions for the unknown compound were chloride and bromide4. The production of precipitate

(Hint the concentration of calcium ions in well 12 is 4.9 x 10-5 M.) Place 5 drops of 0.10 M NaOH in each of the wells 1 through 12. When the NaOH is added to each well, the initial concentrations of the reactants are halved, as each solution dilutes the other. Use an empty pipet to mix each of these combined solutions by drawing each solution up into the pipet and squirting it back into the well. (Hint the concentration of Ca2 ions in well 12 is 2.4 x 10-5 M.) Allow three or four minutes for the precipitates to form, then observe the pattern of precipitation. At one point the concentration of both ions becomes too low to have any precipitate form. We will assume that the first well with no precipitate represents a saturated solution. Part B NaOH varies, Ca(NO3)2 held constant To check your results, repeat the procedure but use a serial dilution of the NaOH. In a different row, put 5 drops of 0.10-M NaOH in well 1. Put 5 drops of distilled water in wells 2 through 12. Add 5 drops of the 0.10-M NaOH solution to well 2. Use an empty pipet to mix the solution by pulling the solution into the pipet and then squirting it back several times. The solution in this well, 2, is now 0.050 M in OH- ion. Continue this serial dilution to well 12, and then remove 5 drops from well 12. Add 5 drops of 0.10 M Ca(NO3)2 to each of the wells, and mix each with an empty pipet or stirrer. Again, determine the well where no more precipitate appears. Cleanup

The purpose of this experiment is to identify the periodic trends in the solubility of the alkaline earth metals and compare the results to that of lead

Introduction: The purpose of this lab was to find the relative solubilities of some salts of the Alkaline Earths and use that information to find the order which they appear in the periodic table; also use that information to efficiently find an unknown alkaline earth halide. Also to find the relative oxidizing powers of the Halogens given and using that information finding the order of the Halogens in the periodic table; also use that information to efficiently find an unknown Halogen.

1. Temperature: high temperature accelerate oxidation, reduction and hydrolysis reaction which lead to drug degradation

In the first test, 0.972g + 0.002g of Na_2 CO_(3(s)) produced 0.354g + 0.004g of CO_2.

When K2CO3 was added to water and CaCl2, the cations of K2CO3 and CaCl2 were switched and due to the solubility rules, the CaCO3 became a precipitate. The KCl is aqueous so we are able to filter out the CaCO3 because the water and potassium chloride and water pass through the filter paper and the calcium carbonate won't because the small holes of the filter paper won't allow the larger molecules of the precipitate to pass through, although the smaller molecules of the water and potassium chloride can pass through. Therefore we don't have to worry about how it will affect our results because it has been filtered out. We didn't have to worry about the spectator ions in this experiment due to the filtering

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