Introduction
Coordination complexes are metals that can accept electron pairs to form coordinate bonds without affecting the charge of the metal. The species that donates its paired electrons is called a ligand. Counterions are not part of the compound but balance the charge of the coordination sphere, the metal and ligands. These compounds are known for their very bold colors and their ability to enhance solubility. In this lab a coordination compound will be formed from Equation 1.
(Equation 1)
From this, the exact formula for the coordination compound can be found using several methods. To find the amount of iron (III) spectrometry will be used. When iron is mixed with sylic acid it makes a deep purple color by measuring the absorbance of the mixture the mass of iron can be found using Equation 2.
(Equation 2)
The mass percent of iron can then be found using Equation 3.
(equation 3)
The amount of oxalate can be found by using titration with potassium permanganate also seen in Equation 1. Using stoichiometry and the concentration of the titrant the mass percent of oxalate can be found using Equation 4.
(Equation 4)
In summary, the purpose of this lab is to synthesize a coordination compound using iron (III) ions, oxalate ligands, and potassium counterions. From this The exact formula for the coordination compound can be found
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50 mL of deionized water and 6 mL of 6.0 M h2so4 was also added. This was repeated two more times for a total of three flasks. A flask was placed on a hot plate and heated until it was at 80 C. As the solution was heated a burette was filled with a KMno4 solution. After the solution was at the required heat a magnetic stir bar was added to create a whirlpool. The KMno4 was then titrated into the solution until the heated solution turned light pink in color. This process was repeated for the two other flasks. The average molarity was then found for the kMno4
The purpose of this experiment was to examine how the stoichiometry, “the quantitative relationships between substances involved in a chemical reaction”, can be applied to determine the quantity of sodium hypochlorite found in a bleach product. This experiment allowed it to determine how much oxidizing agent is in a cleaner by using a redox reaction, which is a reaction involving the transfer of electrons from the compound being oxidized to the compound being reduced. To determine the amount of oxidizing agent, it is necessary to accurately measure out known amounts of redox reactants, know the stoichiometry
This paper describes the methods used in the identification, investigation of properties, and synthesis of an unknown compound. The compound was identified as calcium nitrate by a variety of tests. When the compound was received, it was already known to be one of twelve possible ionic compounds. The flame test identified the presence of the calcium anion in the compound. The compound tested positive for the nitrate cation using the iron sulfate test. At this point it was hypothesized that the compound was calcium nitrate. Reactivity tests and quantitative analysis comparing the unknown compound with calcium nitrate supported this hypothesis. Synthesis reactions were then carried out and analyzed.
We were assigned a group and instructed to measure the amount of different ions in that particular fertilizer sample by counting to preform tests. We used the formula SO4 + Agent —> Percipitat + others. Our job was to add 0.25 g of a fertilizer sample to 100 mL of water to dissolve, then add the agent Pb(NO2)3 to the water also, then filter and dry the water, and distinguish the mass. The was accomplished by using the % formula Mass SO4 = Mass Pb(NO3)2 x MW Pb(NO3)2/ MWPb(NO3)2 to gain the percentage, the the formula Mass SO4/MW SO4 =
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
Experiment: First prepared a well plate with the appropriate amounts of distilled water, HCl, and Na2S2O3 in each well according to the lab manual. The well where the reaction
Kim, Taewoo, Trey L Arnold, Kyle A Leland, Aimee M Morey, Department of Chemistry, USAF Academy, CO 80840
Since the discovery of cisplatin, thousands of platinum complexes were evaluated, but only five were approved. Consequently, more than 10000 compound need to be screened so as to get a novel and more effective anticancer drug than cisplatin with the aid of inorganic or coordination chemistry. Solubility, reactivity, electronic and steric effects, and the configuration of metal complexes can be controlled by modifying the metal to other transition metal such as Pd and Ni or the ligand around the metal atom which has been reported that both the metal and the ligand can determine the biological activity. Hopefully we can find more efficient drugs that may contain much less side effects than cisplatin, as well as solve the problem of overcoming drug resistance of some cancers to cisplatin.
Titrate the solution until the reddish pink color appears. Record the final reading, and calculate the change in volume. Part C. Determination of the molar mass of unknown acid Repeated the procedure above, but this time KHP was replaced with an unknown acidic solution and concentration. Demand the number of replaceable hydrogen from the instructor. Conclusion and Discussion:
Varying the n value carries out the experiment. Absorbencies of each of the ZLn complexes are obtained. The sum of the concentrations of the metal, Z, and the ligand, L, are kept equal. With the ratio of the ligand to the metal in the solution with the maximum absorbance for the ZLn complex, the value of n can be determined as well as the composition of ZLn.
Thickett, Geoffrey. Chemistry 2: HSC course. N/A ed. Vol. 1. Milton: John Wiley & Sons Australia, 2006. 94-108. 1 vols. Print.
Flasks were labelled A to D (refer to appendix 1) 2. 80 mL of tap water was added (neutral pH only) to each flask, where they were placed in beakers at following conditions: Flask A – in ice bath. Flask B – at room temperature. Flask C – in 40 C water bath. Flask D –in 80 C water bath.
tube. Add 6 mL of 0.1M HCl to the first test tube, then 0.1M KMnO4 and
In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143).
Figure 1: The hexacyanoferrate iron (III) ion: contains 6 ligands which are bound to the central metal therefore has a coordination number of 6 (n=6¬). (Hussain,2007) [13]
When a metal cation (M) reacts with a ligand (L) a complex forms. The ligand acts as a Lewis base in the reaction and forms a coordinate covalent bond as the ligands lone pair goes to an empty orbital within the metal. To illustrate this: xM + yL → MxLy where x and y are stoichiometric ratios. To determine the ratios it is possible to use Job’s method. Also known as continuous variance, Job’s method carefully used reactant mixtures such that the total moles and volumes of reactants are constant [Harris, 2010].When just enough of the metal and ligand react the most product is formed. Measuring the absorbance of each solution, the absorbance can be plotted versus a mole fraction of metal or ligand. Using the two resulting equations the mole ratio can be determined. Absorbance is measured by ultraviolet-visible spectroscopy. This method uses visible light and ultraviolet light to excite an electron within a molecule. This will release a photon colored as what colors the molecule doesn’t absorb as the electron returns to its previous energy level. The UV-vis spectroscopic machine then uses this to measure absorbance [Misra 2002]. In this experiment, iron (II) will react with 1, 10-phenanthroline (shown below) to form iron (II)-phenanthroline. This reaction is shown as: