Synthesis and Characterization of K2[Ni(CN)4] , K3[Fe(C2O4)3] and Cu(acac)2 complexes(IV , V and VI) with different structures and Properties 1. Introduction The aim of this experiment was to synthesize HgCo(SCN)4 , [Ni(en)3]S2O3 , NiCl2(PPh3)2 , K2[Ni(CN)4] , K3[Fe(C2O4)3] and Cu(acac)2 but only K2[Ni(CN)4] , K3[Fe(C2O4)3] and Cu(acac)2 were synthesized and explained in this report. Characterization was then done on each of the 3 synthesized complexes by obtaining their UV-Vis spectrum. The UV-Vis spectrum of each complex would identify different properties and would help to explain the observations made when they were synthesized (for example their colour and how they reacted). 2. Method Table 1: Synthesis of K2[Ni(CN)4] Amount of Reagents used Method Observations NiSO4 • 7H2O : 6.00 g KCN : 3.01g In 20ml water NiSO4 • 7H2O was dissolved and the solution containing KCN (dissolved in 7ml water) was added to the Nickel solution. This solution was filtered and the precipitate was washed with small quantities of water. This precipitate was added to the solution of KCN (dissolved in 3ml of water). This solution was heated and swirled so that the crystals that formed dissolved. It was heated again and left so that crystals started forming again. This solution was then placed in an ice bath to enhance crystallization and the crystals were removed by filtration. The water was removed by drying the crystals in the oven at 100°C. A small amount of the sample was dissolved in water and the UV-Vis spectrum was obtained. Nickel (II) sulphate hexahydrate was used in place of heptahydrate. When the precipitate was added to the KCN solution, it turned dark red. As it was heated it darkened even more but as the crystals started forming the colour changed to a light red. As the crystals dried more its colour changed from light red-orange to a light yellow colour. These crystals were dissolved in water for the UV-vis spectrum. The solution was a yellow colour. Table 2: Synthesis of K3[Fe(C2O4)3] Amount of Reagents used Method Observations (NH4)2Fe(SO4)2 • 6H2O: 5.03g To a solution of (NH4)2Fe(SO4)2 • 6H2O (dissolved in 20ml water) 1 ml of sulphuric acid was added and stirred. The oxalic acid (dissolved in 25ml water) was also added and this combined solution was slowly heated to boiling, resulting in the formation of yellow iron(II) oxalate precipitate. The liquid was decanted and 15ml of hot water was added again to the precipitate, this was stirred and filtered. The precipitate (iron(II) oxalate) was transferred to another beaker and a potassium oxalate solution (dissolved in 10ml hot water) was added.
The purpose for this experiment was to determine why it was not possible to obtain a high percent yield when Calcium Nitrate Ca(〖NO_3)〗_2 with a concentration of 0.101 M was mixed with Potassium Iodate KIO_3 with concentration of 0.100 M at varying volumes yielding Calcium Iodate precipitate and Potassium Nitrate. Filtration was used to filter the precipitates of the solutions. The percent yield for solution 1 was 87.7%, and the percent yield for solution 2 was 70.8%. It was not possible to obtain a high percent yield because Calcium Iodate is not completely soluble and some of the precipitates might have been rinsed back to the filtrates when ethanol was used to remove water molecules in the precipitate.
The purpose of the Unknown White Compound Lab was to identify the unknown compound by performing several experiments. Conducting a solubility test, flame test, pH paper test, ion test, pH probe test, conductivity probe test, and synthesizing the compound will accurately identified the unknown compound. In order to narrow down the possible compounds, the solubility test was used to determine that the compound was soluble in water. Next, the flame test was used to compare the unknown compound to other known compounds such as potassium chloride, sodium chloride, and calcium carbonate. The flame test concluded that the cation in the unknown compound was potassium. Following, pH paper was used to determine the compound to be neutral and slightly
At this point the identity of the unknown compound was hypothesized to be calcium nitrate. In order to test this hypothesis, both the unknown compound and known compound were reacted with five different compounds and the results of those reactions were compared. It was important to compare the known and unknown compounds quantitatively as well to ensure that they were indeed the same compound. This was accomplished by reacting them both with a third compound which would produce an insoluble salt that could be filte...
The technique used to narrow down the identity of unknown white compound were solubility test, pH test, flame test, and ion test. The first technique used to narrowed the properties of unknown white compound was using solubility test. To conduct solubility test, 0.25 gram of unknown white compound was dissolved in 100 mL of water. After carefully observing the change while string unknown white compound in water, the unknown white compound was soluble because it dissolved in water completely. Using bursen burner, matches and deionized water, flame test was conducted for unknown compound and it burned lilac color. Then compared the color of unknown white compound to other compound that were narrowed. The results of flame test for compounds that were narrowed down is shown in the following table. The pH test was conducted using litmus paper. 0.50 gram of unknown white compound was measured and dissolved in 10 mL of water in beaker. After dissolving, placed the litmus paper in solution and recorded the pH value of unknown compound which was neutral. Then compared the pH value of unknown white compound to compound that were narrow down. The pH result of the KCL, KNO3, NaCl, and K2SO4 is presented in the following table. The ion test was also conducted in order to make sure that the identity of unknown white compound was matched with the compound that were narrow down. After conducting the test, the result of unknown white compound which formed precipitate compared to KCl, KNO3,NaCl, and K2SO4. The results shown in the following
Triphenylmethyl Bromide. A 400 mL beaker was filled with hot water from the tap. Acetic acid (4 mL) and solid triphenylmethanol (0.199 g, 0.764 mmol) were added to a reaction tube, with 33% hydrobromic acid solution (0.6 mL) being added dropwise via syringe. The compound in the tube then took on a light yellow color. The tube was then placed in the beaker and heated for 5 minutes. After the allotted time, the tube was removed from the hot water bath and allowed to cool to room temperature. In the meantime, an ice bath was made utilizing the 600 mL plastic beaker, which the tube was then placed in for 10 minutes. The compound was then vacuum filtered with the crystals rinsed with water and a small amount of hexane. The crude product was then weighed and recrystallized with hexane to form fine white crystals, which was triphenylmethyl bromide (0.105 g, 0.325 mmol, 42.5%). A Beilstein test was conducted, and the crystals produced a green to greenish-blue flame.
Luminol is a yellow, crystalline compound that has the molecular formula C8H7N3O2. Luminol has unique properties because it exhibits chemiluminescence in low light conditions when exposed to an oxidizing agent. Chemiluminescence occurs when a chemical reaction releases energy in the form of photons. It usually occurs when an oxidizer such as peroxide reacts with an other molecule. The product produced in the reaction is in the excited electron state. When it falls to the ground electronic state, energy is emitted as a photon, which is why light is observed.
8. Continue stirring. Record the temperature at which crystals begin to appear in the solution.
It is made mostly of copper carbonate. It can be crushed into a green powder. If this powder is heated it changes colour. A new substance has been made. The new substance is a black powder.
The metal Ni2+ and the ligand ethylenediamine (en) are studied in this experiment. Solutions are prepared with varying compositions of Ni(en)n2+. Using the equilibrium constants, it is possible to identify which species is present. If the constant for the formation of a species where n is 2 is larger than a species whose constant equals 3 then the former species is pre-dominant. Jobfs Method is limited in that it will give non-integral values of the n present if a fourth complex, ZLn+1, exists. If there is a large variation between the equilibrium constants then only two complexes will be present in the prepared solutions. The absorbance values are plotted, then the value of n can be calculated.
In our experiment we utilized the hydrate cobaltous chloride. Hydrates are crystalline compounds in which one or more molecules of water are combined with each unit of a salt. Cobalt (II) chloride hexahydrate is an inorganic compound which is a deep rose color in its hydrated form. As an inducer of
Mixed melting point was used to confirm the identity of the product. The smaller the range, the more pure the substance. When the two substances are mixed; the melting point should be the same melting range as the as the melting range obtained after filtering. If the mixed melting point is lower one taken from the crystals, then the two substances are different.
Thickett, Geoffrey. Chemistry 2: HSC course. N/A ed. Vol. 1. Milton: John Wiley & Sons Australia, 2006. 94-108. 1 vols. Print.
50 ml of glycerol and 50 ml of distilled water was added inside an Erlenmeyer flask. It was heated to 60 Celsius. NaOH solution was added gradually drop by drop until rose color was observed.
The Solubility of Potassium Nitrate Aim To investigate how the solubility of Potassium Nitrate is affected by Temperature. Background Knowledge Potassium Nitrate (KNO3) is an ionic compound. The strong ionic bonds hold the compound in an ionic lattice which gives KNO3 its crystalline structure. These ionic bonds also have other properties which will affect my investigation, I must be aware of these properties for greater accuracy in my method.
V. Amarnath, D. C. Anthony, K. Amarnath, W. M. Valentine, L. A. Wetterau, D. G. J. Org. Chem. 1991, 56, p. 6924-6931.