Sulfuric acid

3-methylcyclohexene is simple distillation where dehydration was used to prepare the final product. The results of the experiment showed that the 3-methylcyclohexene was formed via an E1 reaction from 2-methylcyclohexanol with a 1:1 ratio of sulfuric acid and phosphoric acid. However, some H2O was left over, which was seen when we look at the IR and see a small water peak. This could be due to the fact that not enough sodium sulfate was added and not for long enough. These results were confirmed by the quality

(a) When dry pH paper was placed over household ammonia, the paper quickly turned a dark blue, indicating that it was a base. (b) When moist pH paper was placed over household ammonia, the paper turned dark blue faster than when dry, still indicating that it was a base. (c) When pH paper was placed over bleach, the paper turned blue, which indicated that it was a base. (d) When pH paper was over ammonium carbonate, the paper turned dark blue even faster than the moist paper over household ammonia

In this experiment, we alkylated P-dimethoxybenzene using tert-butanol and sulfuric acid in order to find the major product of the reaction. Through this experiment, we obtained about 390.2 mg product which equates to about 88.85 percent yield. This yield is very high, even in comparison to alkylations conducted by other undergraduate students such as Jonathan Melville who had a yield of 62% (1). Furthermore, the melting range was 76-85°C, differing from the reference melting point of 102-104°C by

Upon entering the village of DePue, IL, one may ponder about the festering odor of sulfuric acid in the air that clashes with the scenic view of a serene lake surrounded by wooded land. The main street of DePue is lined with locally owned businesses, along with abandoned, crumbling buildings. The community members of this village may either smile and wave at a passer-by, or glare at you with an off-putting facial expression. Despite the confusing impression a non-resident or visitor might form, DePue

Saccharification of Pineapple Ananas comosus peelings through Dilute Acid Hydrolysis Rhoy M. Capul Ma. Michelle Carmel O. Aquino Alia Jenine S. Caceres San Pablo City National High School San Pablo City Mrs. Glory M. Serrano Research Adviser A Science Investigatory Project in fulfillment of Research project S.Y. 2010-2011 Abstract The pineapple is one of the leading products in the Philippines, as it thrives in tropical climates. However

After going through multiple reactions with nitric acid, sodium hydroxide, heat, sulfuric acid, and magnesium, the metallic copper was regenerated. The starting 0.021g of copper changed from solid to liquid to solid to liquid, and finally ended at a solid state. The original copper was 0.021g and the ending copper was 0.008g creating a 38.10% recovery. Results + Calculations: During the lab the staring copper reacted with 10 drops of nitric acid, creating a dark green liquid. Distilled water was

will be explaining the use of ‘superphosphate’ in our local community and how it helps in the process of fertilising. The fertiliser made by using local rock containing fluorapatite( referenced from instruction sheet ) which is combined with sulphuric acid resulting in the solution of ‘superphosphate’ being formed. Also we will be discussing how ‘superphosphate’ affects the community and the environment surrounding it, alongside how is produced and the by-products formed and the effects of these by-products

Acidic Environment Oxides of non-metals which act as acids Non-metals burn in air or oxygen to produce acidic oxides. The addition of water to soluble oxides produces acidic solutions. Oxides of non-metals which act as acids include: * Carbon reacts with oxygen when burnt to form carbon dioxide which is acidic in nature. When dissolved in water, it becomes H2CO3 (carbonic acid). CO2 (g) + H2O (l) →H2CO3 (aq) * Sulfur burns in oxygen to

In the final part of phase one which was steps 9-11, five different metals were placed in Hydrochloric acid. The five metals were copper, magnesium, lead, iron and zinc. Magnesium was the first to react and it created bubbles before it completely dissolved in the acid. Zinc was extremely reactive and produced a lot of bubbles. Iron started reacting after zinc and created some bubbles. Then slowly lead had produced a few bubbles and

elemental form after a chain of reactions. This experiment is very dangerous because of the reactions between the strong acids and bases. In this experiment I performed a series of reactions starting with copper metal and nitric acid to form copper (II) nitrate. Then I reacted copper and several other solutions such as, sodium hydroxide, sulfuric acid, ammonium hydroxide, and hydrochloric acid to form precipitates. In conclusion my percent recovery

positive charge. Stage two Figure 2. Stage 2 of the nitration mechanism The second stage involved a hydrogensulphate ion, HSO4-, which was produced at the same time as the NO2+ ion. This removed a hydrogen from the ring to form sulphuric acid - the catalyst had therefore been regenerated. The electrons which originally joined the hydrogen to the ring were now used to re-establish the delocalised system. Table 1. Observations from the experiment proper Observations: 89 mL conc. H2SO4

the lead in the clean-up. It was easy to identify the hazards: contaminated water, contaminated soil, possible area collapse, and the lead laced chat piles. To begin the Superfund site cleanup the EPA started with monitoring of the surface water, acid mine water discharge, and

disposable pipettes, a stirring rod, a filter flask, filter paper, a Büchner funnel, distilled water, a watch glass, and litmus paper. The chemicals used in this experiment include 6M of HNO_3 (Nitric Acid), 6M of NaOH (Sodium Hydroxide), 3M of H_2 SO_4(Sulfuric acid), 6M of HCl (Hydrochloric Acid), Zinc, and Copper turnings. The experiment began with setting up the first apparatus by placing the 50 mL beaker on the hot plate and attaching the beaker to the ring stand. Then a fume hood was

after six months the emission rates slowly declined. The CO2 and H2O vapour released during eruptions does have a marginal effect on the climate, but by far the most influential gases on Earth’s climate are the sulfuric gasses released. Effects of Volcanic SO2 on Climate The most common sulfuric gas released from volcanic eruptions is SO2. The effect that SO2 has on climate is much more complicated than other volcanic gasses such as CO2 and H2O vapour. SO2 also affects Earth’s climate much more severely

investigation will argue that the Vitamin C level in Golden Circle Pineapple juice will decrease over time. Chemical information and safety surrounding the use of these substances. Previous scientific work: CHEEKY NANDOS Vitamin C: Vitamin C (ascorbic acid) is a water-soluble vitamin, which is needed by the body to form collagen in bones, cartilage, muscle, and blood vessels. Dietary sources of vitamin C include fruits and vegetables, particularly citrus fruits such as oranges. Severe deficiency of vitamin

the crude product is washed with sulfuric acid, water, and sodium bicarbonate to remove any remaining acid or n-butyl alcohol. The primary alkyl halide halide n-butyl bromide is prepared by allowing n-butyl alcohol to react with sodium bromide and sulfuric acid. The sodium bromide reacts with sulfuric acid to produce hydrobromic acid . Excess sulfuric acid acts to shift the equilibrium and speed up the reaction by producing a higher concentration of hydrobromic acid. The

Abstract The concentration of ethanol in vodka was determined by back titration. A known amount of excess potassium chromate was added to the vodka sample to convert ethanol into acetic acid by oxidation. The amount of leftover chromate was determined by titration with iron (II) solution, prepared from dissolution of ferrous ammonium sulfate. Using the amount of chromate added to the vodka solution, the amount of chromate reacted was determined and used to find the amount of ethanol in the sample

many of the pieces have broken down. The beaker was rinsed with 10 mL of distilled water after the mixture was poured through the Büchner funnel of the aspirator. The filtrate was put into a clean 250 mL beaker to be added with 20.5 mL of 6.0M sulfuric acid, stirred slowly when added. The reaction was then put into a 1L beaker ¾ full of ice and water to kick start the reaction into making the alum crystals. The stirring rod was used to help activate the crystals. Once the making of the crystals had

Determination of the Composition of Cobalt Oxalate Hydrate Experiment 12 Robbie Kinsey Partner: Debnil Chowdhury Chem. 1312-D TA’s: Russell Dondero & Sylvester Mosley February 9, 2000 Purpose 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. Procedure The powdered cobalt oxalate

Properties & Hazards of Reagents/Products: (all taken from Sigma-Aldrich website) Acetanilide MM = 135.16 g/mol Melting point = 113-115°C Hazards: acute toxicity Sulfuric acid MM = 98.08 g/mol Boiling point = 290°C Density = 1.840 g/mL Hazards: corrosive to metals and skin, serious eye damage Nitric acid MM = 63.01 g/mol Boiling point = 120.5°C Density =