Oxalate Lab Essay

In this Chemistry Lab the main objective is to perform accurate chemical analysis for the quantity of elements and compounds in a sample. There will be a compound made then synthesized. The methods used were acid-base titrations, redox titrations, gravity filtration, and distillation. General conclusions included

The purpose of this lab is to determine the formula of an unknown hydrate. To achieve this, we heated a hydrate over a Bunsen burner to drive out the water. As a result, the anhydrate is left and the data is used to calculate the mole ratio between the amount of anhydride and water. Then the mole ratios are used to calculate the hydration number, which was 4.8, but was rounded to 5 in the formula. The accepted formula is 〖CuSO〗_4∙5H_2 O and the percent of error was 4%.

With these absorbance numbers a concentration curve was constructed and the unknown solution was determined by finding the point of absorbance on the curve.

There are millions of different organic compounds. Most of them are found in mixtures and in order to achieve a pure form they need to be separated, isolated, and purified. However, there are endless numbers of possible mixtures, which make it impossible to have a pre-designed procedure for every mixture. So chemists often have to make their own procedures. The purpose of this experiment was to prepare the student to the real world by them designing their own procedure which will help them understand the techniques of separation and purification better. The goal was to extract two of the components of the

Hypothesis: The stoichiometric ratio of the reactants in the chemical synthesis of the (2, 4-pentanedianato) iron (III) complex ion is 3:1.

The Beers Law calibration experiment used many concentrations of crystal violet solutions. Each of these solutions were test and analyzed in order to determine the absorbance of each concentration The results were than graphed and produced a slope of 1.00E05 with an intercept of -2.21E-02.

6. Fe (NO3)3, Ferric nitrate, is much more active than ferrous. It could be identified by its reddish color and when mixed with thiocyanate, it reveals a “bloody” red color.

Table 2: Addition of KSCN, Fe(NO₃)₃and Na₂HPO₄to Iron (III) Thiocyanate and Change of Direction of Equilibrium

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.

The first reaction involves pyrite rock reacting with oxygen (air) and water to produce dissolved ferrous iron, sulfate, and acidity. The second reaction oxidizes the dissolved ferrous iron in acidic conditions and produces ferric iron and water. The third reaction involves the hydrolysis of the ferric iron to form ferric hydroxide and more acid. The ferric hydroxide is the orangey-red colored solid you see in the water (Juniata College).

Refer to the reaction of iron nails with a copper solution assignment in Module 3, Section assignment 3.4 Part F of the Chemistry 11 course.

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

This experiment initially involved the synthesis of an iron (III) oxalate complex with the general

Ferrous Gluconaten is used to treat iron deficiency, anemia, so basically lack of red blood cells in our body. Ferrous Gluconate we store at room temperature and protect from sun light. Ferrous gluconate is easily absorbed by the body and it is more water soluble comparing to ferrous sulfate. Also ferrous gluconate is less severity of gastro intestinal side effects due to lower elemental iron in gluconate salt. Ferrous gluconate we found in mainly the black olives also in certain types of fruits and vegetables wine and

Then measured the absorbance of blue fractions that are within 5% of before and after the absorbance of the darkest blue one. Repeated the same steps with the yellow fractions, measured them at 440nm.