The experimental started out with the synthesis of VIVO(acac)2. The vanadyl sulfate was dissolve in distilled water and mixed with acetylacetone, which gave a dark blue solution. From the reaction, sulfate anion was present in the solution, which could react with water in the solution to make the acid, hydrogen sulfate. Therefore, the acid had to be neutralized with sodium bicarbonate. Upon adding sodium bicarbonate, the reaction bubbled releasing CO2 gas and the solution slightly increased to a lighter blue color. Upon completion of the reaction, the greenish-blue precipitate was vacuum filtered and weighed. A mass of 0.4194g of VIVO(acac)2 with a percent yield of 24.8%. The percent yield was low, but that was most likely due to not allowing …show more content…
FeCl3∙6H2O was dissolved in water to give an orange solution. Potassium hydroxide was added to the solution until pH of 8. The potassium hydroxide dissociated in solution and the hydroxide ions bonded with the iron precipitating out orange FeOH crystals. The precipitate was collected using vacuum filtration and then added to an acetylacetone solution. The solution was stirred until it became slushy and held at room temperature for 30 minutes with occasional stirring. The solution was then cooled to 0˚C and then collected using vacuum filtration, where 1.2725g of orange FeIII¬(acac)3 was obtained giving a percent yield of 97.0%. The percent yield was high, but that is mostly due to the precipitate being wet. A lot of the product stuck to the glassware and the Buchner funnel resulting in a loss of …show more content…
A third sample of zinc acetate dihydrate was used for benchtop magnetic susceptibility. By using the data from Table 1, the experimental magnet moment (µeff) was calculation using the equations in Appendix A. In the order of zinc acetate dihydrate, VIVO(acac)2 and FeIII(acac)3, the respective magnet moments were determined to be 2.96, 1.20 and 4.73. The data agrees with what would be expected looking at the electronic states of the metal atoms. Vanadium is in the D5 group of the period table so it is had five unpaired electrons in the D-orbital. Since experimentally V(IV) is produced, that means vanadium has a positive four oxidation state reducing its unpaired electrons in the D-orbital to one. For iron, it is in the D8 group and has a positive three oxidation state so it has a total of five unpaired electrons in its D-orbital. Zinc is in the D10 group and is in the ground state, where all its electrons are paired. Since the magnetic susceptibility is measuring the number of unpaired electrons reacting with a magnetic field, the results demonstrate that by an increase in magnetic moments with the increase in the number of unpaired electrons. The only discrepancy with the data is that the two water molecules in the zinc acetate dihydrate wasn’t accounted for in determining magnetic susceptibility. The magnetic moment of zinc acetate dihydrate was higher than
The next day an orange goopy textured product resulted. The extracts were then dried and combined with anhydrous sodium sulfate, then evaporated with dry air under the hood in a warm water bath. The liquid was cooled and had an initial weighing of 0.5887g. It was reweighed several minutes later with a final
A hot plate was preheated to 100°C. A dry 5-mL long-neck round-bottom flask was clamped over an aluminum block placed on the hot plate. Ferrocene (0.09 g), acetic anhydride (0.35 mL), and 85% phosphoric acid was added to the flask in that order of addition. A magnetic stir bar was added to the flask. Solution was stirred and heated for 10 minutes. Flask was removed and allowed to cool to ambient temperature. DI water (0.5 mL) was added and the solution was cooled to 0°C by ice bath. The solution was neutralized with 3M sodium hydroxide dropwise while stirring and cooling. PH was monitor by pH indictor paper. Solid product was isolated by vacuum
We calculated the specific heat of metal one to be 0.39 J/g℃ which correlates to the exact specific heat capacity of element 30 Zinc. For metal two, we calculated the specific heat capacity to be 0.38 J/g℃ which was close to the actual specific heat of element 23 Iron. The specific heat capacity of Iron was 0.45 J/g℃. Our inaccuracy could be a result of not reading the thermometer as accurately as we could have. To improve yield in the future, we could make sure we record more accurate temperatures.
The mass of the dried product was determined and percent yield was calculated. Part II: Characterization of the Green Salt Observing Photoactivity of the Dissolved Complex Ion Approximately 0.2 g of green salt was transferred in a beaker and dissolved in 50 mL of 1 M H2SO4. One-half of the solution was poured in another beaker and placed in the sunlight, meanwhile, the other half was placed in a cabinet with complete darkness and isolation. Color of both solutions were obtained after 0, 5, 15, and 30 minutes.
The original solution once the 1-butanol, hydrobromic acid, and sulfuric acid were added was yellow-orange in color. After distilling the distillate was clear then became partially cloudy. The calculated yield of the product was approximately 5.41%. The calculated yield was low due to a fluctuating temperature during the reaction and possible impurities formed.
We made a solution of deionized water, Hydrochloric acid, and Methyl Orange. We then determined the concentration of the Methyl Orange that was used to make this solution in particular. Five separate solutions
The two most obvious formation of the precipitate were the combinations with the MgSO4. The MgSO4 and NH3 solution became very opaque and the MgSO4 and Na2CO3 turned from liquid to a full solid white substance. The Na2CO3 and CH3COOH did not have as strong of a reaction, however, the precipitates were able to be visualized with in the clear
In this experiment, six solutions will be tested through various methods, such as mixing with various other test solutions to indicate the presence of different cations. These tests will reveal what cations are present by whether or not it produces a precipitant or if the solution changes colors. Chemicals and Materials Required: This experiment employs the use of the following test solutions:
Obtain ~125 mg (exact amount =126mg) of the Iron(III) Ammonium Oxalate Trihydrate (NH4)3Fe(C2O4)3.3H2O, and dissolve it in the DI water to the total value 25mL.
This experiment initially involved the synthesis of an iron (III) oxalate complex with the general formula Kw[Fex(C2O4)y] zH2O. The variables x, y, and z were determined
The Effect of Changing the Concentration of the Limiting Reagent Calcium Chloride Aqueous (g mL-1) Added to Sodium Carbonate Aqueous on the Percent Yield of the Precipitate Formed in Calcium Carbonate and Sodium Chloride, While the Room Temperature (23℃) and Drying Time (23h) is Kept Constant.
Heavy precipitate emerged immediately and solution turned white in color; solution then became opaque and turned light, bright blue in color.
As magnetite is well-researched, multiple factors influence the formation of iron oxide magnetosomes have been identified. The most important factors are the presence of oxygen, and substrates in the form of nitrogen oxides (Bazylinski 2004). MORE
To do this, a hot water bath was prepared and by placing 250 mL of deionized water into a 600 mL beaker and heating it to 70˚C using a hotplate. An Erlenmeyer flask with 70 mL of deionized water was placed into the hot water bath. When the temperature of the hot water bath was at a constant 70˚C, 0.000 g of FeCl3 and 0.000 g of FeSO4· 7 H2O were added to the Erlenmeyer flask. The flask was swirled around in order to dissolve any solid compounds before being removed from the hot water bath. 20 mL of 2.5 M NaOH was then added drop wise to the solution, so that a black precipitate formed. The solution was allowed to cool before being placed in a centrifuge for 5 minutes at 4000 rpm. The supernatant was then removed, and deionized water was poured over the precipitate to fill the centrifuge tube. Once again, the solution was centrifuged for 5 minutes at 4000 rpm, and the supernatant was removed. The remaining solid, which would ultimately harden to form clay, was removed from the centrifuge tube using a spatula and placed in a beaker to dry for 7
1Irving, H and Williams, R. J. P, The Stability of Transition-metal Complexes. 1952, J. Chem. Soc., 1953, 3192-3210 DOI: 10.1039/JR9530003192 http://www.ciens.ucv.ve/eqsol/Inorganica%20II/articulo2.pdf (assessed 20 Oct 2014)