Vanadyl Sulfate Lab Report

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

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 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

Using of spinel ferrites nanoparticles in electromagnetic devices such as memories, sensors and data storage in modern information technology applications [1-3] made many researchers all over the world do all efforts for synthesis and development of magnetic nano-particles. These nano-particles possess special magnetic and electrical properties with high

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:

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.

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.

The product was precipitated out and isolated using vacuum filtration after 30 minutes. The product was then left to dry on the vacuum for 20 minutes. The weight of the crude product was 2.924 g. The percent crude yield was then determined to be 98.6%. Please note that the calculation shown in the notebook pages used the incorrect weight of the crude product; therefore obtained the incorrect percent crude yield.

The solution that was left over had a faint yellow color to it. This solution was then cooled in an ice-bath for about thirty minutes in order to start the crystallization process. The crystals were dried through vacuum filtration and put into a vial which was then weighed, showing that 91.67% of the initial substance was

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.

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

Subsequently, 10mL of 3.5% H2O2 were added dropwise to the reaction mixture and was stirred for 20 minutes before heating to boiling at 80°C for 5 minutes. The reaction mixture was then taken off heat and allowed to cool undisturbed in an ice-bath for 30 minutes. Suction filtration was performed after to collect the crystals from the chilled solution The product was then washed with chilled 95% ethanol (2 x 15mL) and followed by diethyl ether (2 x 10mL). The crude product was then left to dry before recording the yield. 20mg of the crude product is then accurately weighed out and dissolved in deionized water in a 25mL volumetric flask. Deionized water was added to the volumetric flask to the mark and the UV-vis absorption spectrum of the crude product was recorded.