Cyclohexanone Lab Report

Marwah Alabbad Post lab 10/21/15 Question 1: 1. Experiment 1: Number of trails NaOH concentration (M) Volume of HCl solution (mL) Initial volume of NaOH(mL) final volume of NaOH(mL) The volume of NaOH to titrate HCl (mL) Concentration of HCl (M) 1st 0.1023 25.0 10.05 36.12 26.07 0.085 2nd 0.1023 25.0 5.74 31.40 25.66 0.105 3rd 0.1023 25.0 9.84 35.52 25.68 0.105 First trail calculation: 0.02607L× (0.1023mole NaOH/1L)×(1 mol of HCL/1 mol of NaOH)×(1/0.025)= 0.085M of HCl

That mixture was then filtered through a coffee filter. Nine test tubes were prepared in order to perform this dye coupled reaction. One contained 5.0ml of the potato and pH buffer mixture, 2.0 ml of hydrogen peroxide, and 1.0 of guaiacol to serve as a blank for the spectrophotometer. Four test tubes were filled with 2.0 ml of hydrogen peroxide and 1.0 ml of guaiacol, used for measurement by the spectrophotometer, each. The last four were filled with 4.0 ml of the potato and pH buffer mixture and 1.0 ml of peroxidase.

The compounds tested in included the unknown, Calcium Nitrate, Calcium Chloride, Calcium Carbonate, Sodium Chloride, Potassium Chloride, Magnesium Chloride, and Ammonium Chloride. The next test was the pH test. In this test, the aqueous solutions from the flame tests were used again. A piece of pH paper was dipped into the aqueous solutions, a different piece for each solution. The ensuing coloration of the paper was compared to the pH scale and the

A: The compound that is being oxidized in the luminol synthesis reaction is Na2S2O4, (Sodium Hydrosulfite. Since sodium hydrosulfite is acting as the reducing agent, in this experiment. 2. What is the purpose of acetic acid in the luminol synthesis reaction? How would the amount of the luminol product obtained at the end of the reaction be affected if the number of moles of NaOH added at the beginning of the reaction and the acetic acid added at the end of the reaction added were reversed?

1. What type of macroscopic evidence for chemical change did you observe during this experiment? Give at least three different examples. (15 points)

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

The oxidation of Cyclohexanone for the

Conclusion: Based on the results of molarity from Trials 1, 2, and 3, it is concluded that our experimental for each trial is .410M NaOH, .410M NaOH, and .450M NaOH. The actual molarity of the NaOH concentration used was found to be 1.5M NaOH. The percent error of the results resulted in 72%. The large error may have occurred due to over titration of the NaOH, as the color of the solution in the flask was a darker pink in comparison for the needed faint pink. Discussion of Theory:

In this experiment, two alcohols, 1-propanol and 2-propanol, were oxidized through combining each with an excess amount of chromic acid solution. The purpose for conducting this experiment was to determine the reaction rate constant at which aldehydes and ketones formed from the respective oxidation of 1-propanol and 2-propanol. From this value, the half-life of the alcohol during the reaction could be derived. The progress of the reaction was tracked through the color change of the solution through use of a spectrophotometer. The first 6 minutes of absorbance of each alcohol’s oxidation were graphed.

The oxidation reaction of ethyne gas is facilitated by potassium permanganate, which is the catalyst in the reaction. The reaction allows ethyne to be oxidized into ethan-1,1,2,2-tetraol by breaking the two pi bonds between the carbons and adding hydroxyl groups. However, the new compound, having 2 hydroxyl groups on each carbon, results in the hydroxyl groups reacting with each other so that two H2O molecules are released and each carbon becomes double-bonded with an oxygen, creating ethandial. The ethandial is further oxidized, through the use of potassium permanganate, to oxalic acid as aldehydes are easily oxidized. No ethandial is preserved as the solution the reaction took place in was not acidic.

There are two methods of obtaining cyclohexane. These two methods are fractional distillation of naphtha and hydrogenation of benzene. Research suggest that the hydrogenation of benzene is the most economical way to create our chemical of choice. According to ICIS, cyclohexane is used in the production of adipic acid used to

This has two important consequences; Aliquat has favorable intermolecular forces that allow it to dissolve in an organic layer while containing a positive charge, and it is able to form a complex with WO42-, which is necessary for the oxidation of cyclohexene. After being carried into the aqueous layer, WO42- can form a complex with cyclohexene that allows a more direct route of oxidation. This reaction also took place in the presence of KHSO4 because the reaction occurs more readily under acidic conditions. Cyclohexene is a hydrocarbon that was able to undergo an addition reaction because of its carbon-carbon double bond. The extra electron density that results from this bond provides an ideal location for a reaction to take place because of its nucleophilic properties, and the need of each carbon to form a new bond once the double bond is broken.

The equation of the reaction between sodium hydroxide and ethanoic acid is as follows: CH3COOH + NaOH → CH3COONa + H2O We can measure the end point of titration process and we can also measure the amount of reactants. The concentration of ethanoic acid in the vinegar can be determined through stoichiometric calculations, Using the values obtained from the titration, and also the chemical equation as a reference. Phenolphthalein indicator is used in this acid-base titration Equipment and materials:

Its pH is greater than 7 and turns red litmus paper into blue. Acid- base neutralization is done by adding an acid to a base or a base to an acid until the substance has equal hydrogen and hydroxide ions. This is used to determine unknown concentration of a

Introduction Strong acids and strong acids both dissociate completely in water forming ions. However, strong acids donate a proton to form H3O+ along with a conjugate base and strong bases accept a proton to form OH- along with a conjugate acid. The chemical behavior of acids and bases are opposite. When they are together, their ions cancel out and form a neutral solution. In this experiment, HCl and NaOH will react to form NaOH and H2O with these two steps: The overall reaction is: Both Na+ and Cl- ions combine to form NaCl.