The Aromatic Substitution : Preparing Methyl M Nitrobenzene

(.1063 KIO31) (1 mol KIO214 g) x 6 mol S2O41 mol KIO= .00298.04150= .259 M

2) (0.3 g NaBH4 x 154.16 g ethyl vanillyl alcohol) / (37.83 g NaBH4) = 1.223 g ethyl vanillyl alcohol

The objective of the experiment was to reduce Benzil, using sodium borohyride as the reducing agent. In a benzil reduction, there are five possible products than can occur, specifically a racemic mixture of benzoin, racemic mixture of hydrobenzoin, or meso-hydrobenzoin. Therefore, three different tests were conducted in determining the identity of the product: melting point, thin light chromatography, and infrared spectroscopy.

H. How would you prepare 10 mL of a 0.25M HCl solution if 1M HCl was available? How much

7. To each fresh tube of alcohol, 2 mL of 0.01 mol/L KMnO4 was added, and step 4. was repeated.

(0.074 mol HCl x 1 mol NaOH) / 1 mol HCl = 0.074 mol NaOH

For each of the 3 acceptable trials, enter the precise volume in milliliters of sodium thiosulfate solution used in

Water MW=18.01 H2O MP= 0.00 BP= 99.98 1.0 soluble none (1R)-(+)-Camphor MW= 152.23 C10H16O MP= 179-181 °C BP= 204 °C 0,99 g/cm3 1.2 g dm−3 Highly flammable, Harmful, irritant Sodium Borohydride MW= 37.83 NaBH4 MP= 400 °C BP= 500°C 1.035 g/mL at 25 °C soluble Highly Flammable, harmful, toxic, corrosive Methanol MW=32.04 CH4O MP= -98 °C BP= 65.4 °C 0.791 g/mL at 25 °C

molality m= (grams MgCl2÷95.21gmol of MgCl2)10mL H2O×1g H2O1 mL H2O×1 kg H2O1000 g H2O+grams of ice×% of ice melted×1 kg ice1000 g ice

3.6.3. 2, 4 – D (2, 4–Dichloro phenoxy acetic acid) stock solution (1mg/ml): 10.0mg of 2.4-D being weighed and dissolved completely in 1N NaOH to a final total volume

Aromatic compounds can undergo electrophilic substitution reactions. In these reactions, the aromatic ring acts as a nucleophile (an electron pair donor) and reacts with an electrophilic reagent (an electron pair acceptor) resulting in the replacement of a hydrogen on the aromatic ring with the electrophile. Due to the fact that the conjugated 6π-electron system of the aromatic ring is so stable, the carbocation intermediate loses a proton to sustain the aromatic ring rather than reacting with a nucleophile. Ring substituents strongly influence the rate and position of electrophilic attack. Electron-donating groups on the benzene ring speed up the substitution process by stabilizing the carbocation intermediate. Electron-withdrawing groups, however, slow down the aromatic substitution because formation of the carbocation intermediate is more difficult. The electron-withdrawing group withdraws electron density from a species that is already positively charged making it very electron deficient. Therefore, electron-donating groups are considered to be “activating” and electron-withdrawing groups are “deactivating”. Activating substituents direct incoming groups to either the “ortho” or “para” positions. Deactivating substituents, with the exception of the halogens, direct incoming groups to the “meta” position. The experiment described above was an example of a specific electrophilic aromatic

Purpose: The purpose of this experiment is to synthesize methyl nitrobenzoate from methyl benzoate, concentrated nitric acid, and concentrated sulfuric acid via an

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In this experiment, methyl benzoate was synthesized from benzoic acid and methanol with acid catalyze using Fisher Esterification. First benzoic acid and methanol were mixed in 100 mL round bottom flask. We cooled the mixture in ice and poured 3 mL of conc. H2SO4 and swirled to mix compounds. Then we refluxed the mixture for 1 hour. We let the solution cool and then decanted into a separatory funnel containing 50 mL of water and rinsed the round bottom flask with 35 mL of tert-butyl methyl ether and added that to a separatory funnel. We shook and vented thoroughly and drained the aqueous layer which contained a bulk of methanol and H2SO4. We washed the solution in the separatory funnel with 25 mL of water, followed by 25 mL of sat. sodium bicarbonate

4g of Na CO x 1 mol of Na CO 4g of CaCl x 1mol of CaCl