Cobalt Synthesis Lab Report

Aspirin Recrysalization Data Table Actual Mass (g) 0.41 Actual MP (ºC) 123-125 Expected Mass (g) 0.533 Expected MP (ºC) 135 Percent Recovery 77% Percent Error 8%

Overall, the experimental results were similar to the results needed to identify the cobalt ammine halide coordination complex. The color of the compound was dark purple and it looked just as expected as the experiments leading up to the collection of the synthesized cobalt compound had little to no errors. The percent yield of the compound was not 100% due to small errors throughout experiments such as losing some of the compound during transferring, more liquid evaporating than desired, and not measuring volume to exact accuracy and precision every time. For example, when the graduated cylinder was filled with 100 mL deionized water and the liquid was poured into a flask, the liquid measured over the 100 mL mark on the flask, meaning that

The purpose of this lab was to determine the percent cobalt and oxalate by mass, and with that information, the empirical formula for cobalt oxalate hydrate, using the general formula Coa(C2O4)b.cH2O.

When combined Sodium Bicarbonate and Hydrochloric Acid, Carbon Dioxide is produced. The two chemicals do not undergo a change in color but a chemical change when CO2 is produced.

I started with elemental copper metal and then reactions occur step by step as follows:

The goal of the experiment was to determine the unknown concentration of the provided Cobalt (II) solution by using a spectrophotometer/colorimeter. The spectrophotometer was used on the unknown solution to find the concentration of Cobalt (II). The concepts used from Beer-Lambert’s Law are the absorbance and concentration of the tested solution. The equation is A=EbC. A equals absorbance, E is the constant when identifying the species measuring the wavelength, b is the thickness of the solution, and C is the concentration of the solution. E and b are both constant, which makes the concentration and the absorbance directly proportional. Results resembled the standard curve and the connection of absorbance and concentration was used to estimate

In this lab, the purpose is to get a piece of copper back to copper with the same physical properties and mass through multiple reactions with different reactants. The law of conservation of mass ties into this experiment because the law of conservation of mass where the mass stays the same no matter what happens to it because nothing gets destroyed or created; nothing can just disappear. Instead, the matter has changed into another state of matter. Additionally, the reactants’ mass and the products’ mass should be equivalent when it comes to reactions. However, that isn’t always the case because margin of errors can happen that can affect the law of conservation of mass, which is why I believe the copper will be able to get back to the initial

A general increase in absorbance values is seen in all three curves. All curves plateau at various temperatures. The absorbance was taken at 260nm. Temperature values ranged from 70°C to 96°C.

Cobalt was discovered by a Swedish chemist by the name of Georg Brandt. In 1735, Georg was trying to prove that certain minerals had the ability to color glass blue and was not due to bismuth but due to an unknown element (1). Since then, it has developed into a highly useful isotope.

Cobalt has many uses in the aspect of Chemistry. One of the main uses is a catalyst in petroleum. Specifically, CoMoO4 is used to help change petroleum into gas (Newton). This chemical removes the sulfur in the oil to make it a useable fuel source. Also cobalt is used as a catalyst to speed up the resin process when making plastics (Cobalt Facts). Cobalt is also used to produce bright blue colors in paints (Cobalt Periodic). They are also in many other chemical dyes and paints and they can help determine how quickly these paints dry which can be very important to artists (Cobalt Facts). They are also used in dyes for glass, glazes, cosmetics, inks, and pottery (Newton). Here is a chart on chemical

The solution changed colour because, we added a reactant which means the forward reaction will occur faster than the reverse, which means there will be more products formed than reactants, because the reverse reaction is slower. The tube would feel slightly colder, because the reaction consumes the heat, and moves in the endothermic direction. Cobalt system Action Observation Shift Explanation heat Turns blue left When heat is

This paper examines material based on Beer Lambert’s law and spectrophotometry. It shows what happens between the concentration and absorbance of CoCl2 x 6H20 (Cobalt (II) Chloride Hexahdrate). To detect the wavelength and unidentified solution , the spectrophotometry was employed. After everything, in a proper graph we gathered the the data to demonsrate what relationship absorption and concentration have. Moreover, Spectrophotometer, electromagnetic, lambda max were considered to make the experiment a success. A spectrophotometer measures the intensity of light through a unknown solution. The methodology will give you a brief discription of the way the experiment was perfomed. The main ambition of this lab will be demonstrated with the experimental result. All labs were were put into a grap and table. Therefore errors that occurred throughout the lab were explained and what should be done in the future to make a acknowleged lab.

Abstract: Through a series of substitution reactions, different cobalt ammine complexes were created. These complexes were analyzed via, precipitation and gravimetric measures to determine that the substitution reactions that occurred.

The compounds of the transition metals react with negative ions and/ or neutral molecules to form transition metal complexes. Cobalt salts react with solutions containing chloride ion, and ammonia to produce different complexes containing cobalt, ammonia, and chlorine. A handout called “The Cobalt Complex Project-Synthesis” was given by the instructor. The experiment was carried out according to the detail directions written on the paper. The color of the solution didn’t change after dissolving ammonium chloride in concentrated aqueous ammonium hydrioxie. The solution’s color started changing after putting cobalt(II) chloride hexahydrate. While adding the concentrated aqueous hydrogen peroxide, the effervescences were formed. The color of the

Picture C. Shows the difference in color of CoCl2 + concentrated HCl when placed in different temperatures.