Ion exchange

The unknown NMR/IR Unknown #7 was C8H11N. The first in determining the structure from looking at the NMR spectra was to determine the degrees of saturation (DoU). DoU helps identify the number of bonds within the compound. The DoU can be determined by looking at the chemical formula and using the equation, DoU= (2C + 2 + N - X – H)/ (2). For this particular compound, I identified that the DoU was 4. Next, using the given IR peak, as well as looking at the chemical formula, the weak wavelength of

cations and anions in an unknown salt. 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

Silver nitrate is corroding your copper pipes. Would running sodium chloride through your water system stop the corrosion from happening? What are ways to prove the presence of silver nitrate in your system initially? The corrosion of copper and silver nitrate is a single replace chemical reaction seen in the chemical formula: 2AgNO3(Aq) + Cu(S) → Cu(NO3)2(Aq) + 2Ag(S) The reactants in this reaction are silver nitrate and copper, and the products are copper nitrate and silver. How would you prove

Water is one of the essential components that are a prerequisite in supporting life. It can be described as an odorless, tasteless and transparent liquid that occur naturally. Water is colorless when it is in small amount, but adopts a bluish color when it is in large quantities. As a natural compound, water is the most abundant and familiar liquid that exist on earth. In its natural solid (ice) and liquid form, water is estimated to cover over 70% of the entire surface of the universe (Sikorski

small error. And not only that but also the fact that as table 2 shows that the final amount needed was .0131 g less to the actual mount that we added from table 1. During the procedure our percent error must of have come from loosing the silver ions. After heating we had to wash the moisture of the watch glass back into the beaker and there could have been a possibility that we didn’t wash of all of the silver back into the beaker. When it precipitated, some of the particles may have peptized

In Part A of the experiment, the Unknown Substance #4 was found to contain Silver. Since no precipitate was formed in Step 6 of the experiment, it was confirmed that there was no presence of lead. Step 8 verified that the unknown solution contained Silver, with the formation of the white AgCl precipitate. Silver was reasonable since it was confirmed that it was not Lead. Part B of the experiment resulted in the identification of Barium. The presence of Barium was confirmed in Step 13, with the formation

In this experiment, there are no significant ethical considerations as we had not used any living organisms. There were no extreme safety concerns, however there are still precautions that needed to be taken. Cobalt chloride is very toxic and is irritating to the skin so when handling the cobalt chloride solution, wear lab coats and safety goggles and have all hair tied up. Handle the solution with care to try and prevent the solution from coming into contact with skin. If it does spill onto skin

between aqueous iron ions (Fe3+) and aqueous thiocyanate ions (SCN-) reacting to form aqueous FeSCN2+ was observed.2 Since this process is an equilibrium reaction, it can also proceed in the reverse direction where FeSCN2+ decomposes to form Fe3+ and SCN-. One of the initial starting reactants for this experiment was Fe(NO3)3, which decomposes to form iron ions and nitrate ions. The other starting reactant was KSCN, which decomposes to form potassium ions and thiocyanate ions. Although both decomposition

RESULTS & DISCUSSION The unknown solution of metal nitrate salts was identified to contain silver (Ag+) and Calcium (Ca2). These cations were discovered through a qualitative procedure that systematically separated the unknown ions from the solution by introducing known reagents and observing the resulting reaction that presented characteristic chemical properties unique to each cation. These observations guided the flow of the procedure, with the expected results of each step accumulating to justify

In conclusion, the chemical formula of the dehydrated sample was found to be CuCl2 and the formula for the hydrated sample was CuCl2 ·2H2O. Thorough experimental procedure was taken to obtain the water loss of the hydrated sample, therefore defining its chemical formula. As the hydrated sample of copper chloride changed colors throughout the heating process, a change in chemical composition was noted. The hydrate was originally a blue/green color, but as it was heated and lost its water, the hydrate