In this project, titanium(IV) ethoxide, Ti(CC2H5)4, Cobalt(II) nitrate, Co(NO3)2.6H2O, Iron(III) nitrate-9-hydrates, Fe(NO3)3.9H2O, and strontium nitrate, Sr(NO3)2 are needed to prepare both non-substituted strontium ferrite and substituted strontium ferrite. In this case, non-substituted strontium ferrite acts as a control in this project to compare with the characteristics of cobalt-titanium substituted strontium ferrite. The main objective of this project is to compare the effect of substitution of cobalt-titanium ions to strontium ferrite using the control, the strontium ferrite without any substitution. In order to create a suitable medium for mixing, ethylene glycol is for formation of gel in this projectIn this project, different stoichiometric …show more content…
Throughout the mixing process, the clear red solution slowly changes to a denser red solution (Appendix figure 23). A thermometer was used for temperature checking. The beaker was removed from the hot plate when the temperature was found to be higher than 50 ℃. This was done to prevent a sudden gelation happen before all the active dissolved in the ethylene glycol. Moderate heating of the solution for a period of time is allowed to obtain a wet gel (Appendix figure 24). The wet gel may not look fully solid depending on the composition of the active added into the ethylene glycol. When all the active ingredients were dissolved in the ethylene glycol, the solution turned color from a clear red solution to a darker reddish brown color. The wet gel was observed to be slightly reddish brown in color. Before moving on to the formation of gel process, the magnetic bars were removed from all the samples. Continuous heating at high temperature (more than 50℃ but lower than 80℃) was allowed to obtain wet gel for all the samples of Co-Ti substitution from 0.2 to 1.0. After the wet gel was formed, continuous heating of the wet gel yield the product in powder …show more content…
Magnetic susceptibility and photoluminescence are analyzed after the calcination process using magnetic susceptibility balance (Sherwood Scientific, Appendix Figure 27) and fluorescence spectrometer with excitation wavelengths range from 370 nm to 600 nm, emission wavelength 390, excitation slits set at 5.0 nm and the scan speed of 500 nm/min (PerkinElmer fluorescene spectrometer LS 55, Appendix Figure 28). In the calcination process, the furnace was activated in the morning of the day (around 10a.m) and was off in the evening (at 5p.m). The synthesis of strontium ferrite is using the same pathway by using only strontium nitrate and iron(III) nitrate-9-hydrates. In sol-gel process, this process is a method to establish a sol and allow formation of gel and removal of solvent. The metal or metalloid element is surrounded by different kinds of ligands and they are suspended in the medium called precursors. The organization of the suspended molecules to form bond at random forming a network called gel. In this state, the gel consists a continuous solid skeleton encloses the liquid phase. When the “cluster” extending itself throughout the entire sol, this point is giving a name called “gel
While the solution dissolved, 50 mL of distilled water was added to a 150 mL beaker and heated on the hot plate. When the solution started to boil 2.65 grams of Na2SiO3*5H2O was added to the beaker with a stir bar and heated to a gentle boil. When both solutions began to boil, the sodium silicate solution was slowly added to the sodium aluminate. The solution was kept at 900C for 60 minutes and stirred with stir bar. After 60 minutes, the zeolite solution was cooled for 5 minutes and for the magnetized zeolite , 0.78 grams of FeCl3 and 0.39 grams of FeSO4*7H2O was added to the flask and stirred until the iron parts dissolved.
This layer is virtually invisible as it has a very small thickness and is also transparent. In order to prevent the fogging and dirt on glasses, the coating must be under UV illumination for it to sustain the hydrophobic property. 3.2.2 Methods to fabricate TiO2-SWCNT composite There are enormous methods available to prepare the nanocomposite of CNT and TiO2 which are sol-gel method, electrospinning method, hydrothermal and more. 3.2.2.1 Sol-gel synthesis Sol-gel is a method in which small molecules are used to produce solid materials. The method is used for the fabrication of metal oxides.
Next, about 10 mL of both solutions, Red 40 and Blue 1, were added to a small beaker. The concentration of the stock solution were recorded, 52.1 ppm for Red 40 and 16.6 ppm for Blue 1. Then, using the volumetric pipette, 5 mL of each solution was transferred into a 10 mL volumetric flask, labelled either R1 or B1. Deionized water was added into the flask using a pipette until the solution level reached a line which indicated 10 mL. A cap for the flask was inserted and the flask was invented a few times to completely mix the solution. Then, the volumetric pipette was rinsed with fresh deionized water and
Observations The purpose of this experiment was to be able to synthesize triphenylmethyl bromide from triphenylmethanol by a trityl carbocation intermediate. During the experiment, 0.100 g of triphenylmethanol was placed into a small test tube. The triphenylmethanol looked like a white powder. Next 2 mL of acetic acid was added to the test tube and the solution turned a cloudy white color.
Metal cations can be identified based on the colors they emitted off when heated in a flame.1 When atoms of the ions that were tested are excited, their electrons move up to higher levels of energy.2 When the electrons relax and return to the original states, they emit photons of specific energy creating wavelengths of light that produces colors.3 The test wire and Bunsen Burner were used to excite the solution in the crucible. The standard metal cations that were tested and their outcomes are as shown in Table 1.
In the lab, “Properties of Hydrates,” the purpose was to compare the properties of several well observable hydrates and to determine if dehydration is a reversible or irreversible change. The lab consisted of attaining a pea-size sample of each compound, burning it over a bunsen burner, and comparing the starting mass and the mass lost after the combustion. These results are important to be able to identify a variety of different chemicals that contain water molecules as part of their crystalline structure. Some can be removed by heating (resulting in evaporation) and some remain mostly unchanged. In this lab the answer will be found.
The following lab period the solid was weighed (0.0483 g) and percent yield was calculated (65.5%) with the limiting reagent being tetraphenylcyclopentadienone. The melting point was determined. The first melting point was 204-204.9 °C and the second melting point was 215.6-215.9°C. Finally, an infrared spectroscopy was obtained for the
Glacial acetic acid and acetic anhydride were added to the mixture while refluxing, which converted the lime colored solution into a clear mixture. The flask was cooled in an ice bath and the solution
Abstract: The purpose of this experiment was to identify given Unknown White Compound by conducting various test and learning how to use lab techniques. Tests that are used during this experiment were a flame test, ion test, pH test, and conductivity test. The results drawn from these tests confirmed the identity of the Unknown White Compound to be sodium acetate (NaC2H3O2) because there were no presence of ions and sodium has a strong persistent orange color. The compound then will be synthesized with the compounds Na2CO3 and HC2H3O2 to find percent yield.
- A hydrate is a salt that contains water as a part of its crystal structure. The hydrate used in this lab was Copper (ll) Sulfate Pentahydrate. To heat the hydrate in this lab a crucible is needed. A crucible is a heat resistant container used to heat things to high temperatures. In this lab a mole was used to determine the measurements of all substances.
The Wittig reaction is valuable reaction. It has unique properties that allows for a carbon=carbon double bond to form from where a C=O double bond used to be located. Creating additional C=C double bonds is valuable due to its use in synthesis. The Wittig reaction will allow the synthesis of Stilbene (E and Z) from a Benzaldehyde (Ketcha, 141).
Empirical Formula of Magnesium Oxide - Lab Report Background Information/Introduction: The aim of this lab is to determine the empirical formula of magnesium oxide by converting magnesium to magnesium oxide. As an alkali earth metal, magnesium reacts violently when heated with oxygen to produce magnesium oxide and magnesium nitride as a byproduct. In order to obtain only magnesium oxide, distilled water was added so that magnesium nitride will react and convert to magnesium hydroxide. Further heating then oxidizes all of the magnesium into magnesium oxide.
Introduction: In this lab, of water in a hydrate, or a substance whose crystalline structure is bound to water molecules by weak bonds, is determined by heating up a small sample of it. By heating, the water of hydration, or bound water, is removed, leaving only what is called an anhydrous compound. Based on the percent water in the hydrate, it can be classified as one of three types: BaCl2O ⋅ 2H20, with a percent water of about 14.57%, CuSO4
Paragraph 1 The research paper talks about how the temperature of formation and crystallinity of iron phosphate, FePO4, is critical in determining its electrochemical behaviour. FePO4 is known to crystalline in several different structures. At 600 degrees, FePO4 irreversibly changes into an electrochemically inactive quartz-like structure, which shows that the olivine form is metastable. FePO4 at a high temperature is limited to measurements of call parameters. In the case of α-phase FePO4, cell parameters tend to increase exponentially as temperature increase.
Properties of Ionic and Covalent Substances Lab Report Introduction The purpose of this lab was to determine which of the following substances: wax, sugar, and salt, are an ionic compound and which are a covalent compound. In order to accurately digest the experiments results, definitions of each relating factor were researched, leading to the following information: ionic compounds are positive and negatively charged ions that experience attraction to each other and pull together in a cluster of ionic bonds; they are the strongest compound, are separated in high temperatures, and can be separated by polar water molecules. A covalent compound is formed when two or more nonmetal atoms share valence electrons; covalent compounds are also categorized into two sections: polar covalent and nonpolar covalent. Furthermore, polar covalent compounds dissolve in water, while nonpolar covalent compounds do not.