Hence, a calcium chloride and cotton were filled inside a drying tube. The condenser was wrapped with parafilm and a paper towel to avoid moistures from entering. The reagent will act as nucleophilic addition to acetone and work up with hydrochloride acid to synthesize 2-methylhexanol. Throughout this process, the solution turns dark grey and develop white precipitates. This step indicate that Grignard reagent was generated, and the extra white precipitates were magnesium.
Paragraph 1 The objective of the experiment is to test; how will water temperature affect the rate of reaction of an alka-seltzer tablet? The dependent variable of the experiment is the dissolving time. When an alka-seltzer tablet starts to fizz it begins to dissolve, due to the citric acid and sodium bicarbonate the tablet contains (Clark, “Why does Alka-Seltzer fizz?). When the tablet is in solid form, the two ingredients are not yet mixed together, but by dropping the tablet in water, a chemical reaction is catalyzed between them, creating a fizzing sensation (Clark, “Why does Alka-Seltzer fizz?). When the sodium bicarbonate is placed in water, it begins to split apart and form bicarbonate and sodium ions (Science Buddies, Carbonation Countdown:
The chloroform and caffeine mixture was collected and into a conical flask labeled A. The remainder of the solution was discarded. This was repeated for beakers B and C. 9. Sodium sulphate was then added to each beaker to dry the liquid by getting rid of any remaining water from the solution. The sodium sulphate was then filtered and discarded.
This is what makes it dissolve. Sodium bicarbonate or baking ions react with hydrogen ions then mixes ions with water, carbon dioxide gas which is the fizz. Baking soda and citric acid mixed when dropped in the water, which causes a chemical reaction to happen. There are multiple components that make an alka-seltzer dissolve.
Purpose The purpose of this experiment was to evaluate the stoichiometric relationship between the testing agents and to identify the products formed. The relationship was found by completing three acid and base neutralization reactions using phosphoric acid, which is a triprotic acid, with different volumes of sodium hydroxide. Introduction Procedure Phosphoric acid solution with a volume of 1.00 mL and a molarity of 6.00 M was transferred into a 125-mL Erlenmeyer flask using a volumetric pipette. Sodium hydroxide solution with a volume of 6.00 mL and a molarity of 3.00 M was transferred into a 50 mL beaker using a volumetric pipette. While swirling the phosphoric acid solution in the Erlenmeyer flask, the sodium hydroxide solution was added to it a few drops at a time using a disposable plastic pipette.
Phosphoric acid was used as a catalyst in this experiment to speed up the reaction. Water will be used to quench the excess acetic acid. The product in Aspirin synthesis is not very water soluble which means that precipitate will form when the water is added. Spectroscopy is used in this experiment to determine the presence of the product or “purity” of the product. The synthesis of Aspirin involves the chemical interaction between salicylic acid and an acetyl anhydride which causes a chemical reaction that converts salicylic hydroxyl group in to an acetyl group.
This conversion was required to perform a conjugated addition of the alpha-carbon of acetone to 2-nitrobenzaldehyde, resulting in formation of an aldol, which is subsequently converted to Indoxyl. 5mL of 2M Sodium Hydroxide was diluted by the presence of 35mL of water, effectively reducing its concentration to 0.25M. A low hydroxide ion concentration was required to prevent aldol from condensing, which will result in the hydroxyl group leaving as water. Ethanol was subsequently added to reduce the time required for drying
Aim The purpose of this lab was to separate a mixture of carboxylic acid (p- toluic acid), a phenol (p-tert-butylphenol) and a neutral compound (acetanilide) using solvent extraction. Introduction Solvent extraction is a process that separates compounds from a mixture by a solvent. It involves the transfer of compounds from one liquid solvent to another liquid solvent. The two solvents used in this process should be immiscible to each other for the separation of compounds leading to an organic phase and an aqueous phase. The organic phase is composed of a solvent that is insoluble in water mainly consisting of non-polar compounds.
Used solvents contain contaminants that can be removed by fractional distillation. The recycled solvents have purities suitable for re-use. Fractional distillation is used to separate the crude oil into its various components such as gasoline, kerosene oil, diesel oil, paraffin wax, liberating oil. Fractional distillation is also used for the purification of water. Water contains many dissolved impurities; these can be removed by this process.
Chromic acid is added continuously until a slight brownish colour solution persists, this is to make sure that complete oxidation of borneol in the experiment. Light petroleum was used to dissolve and extract the product from the aqueous layer twice, 15 mL each. Sodium carbonate and saturated solution were used to wash product and separate both aqueous and organic layer in the separating funnel. This is to increase the accuracy when flowing out the aqueous layer. The extracted organic layer was steam bathed to vaporize light petroleum which has low boiling point at 30-40˚C.
Purpose and Techniques: This experiment has the aim to determine a chemical formula of hydrated compound, which ingrains cupper, chloride and water molecules in its structure. In order to find this hydrated compound, it is necessary to use the law of multiple proportions. In other word, finding the appropriate variables values to this compound (CxCly*zH2O). Additionally, two major steps are required to proceed the experiment. The first consists to heat a sample to liberate the water hydration, and then compare two mass weights before and after heating so gets easier to find the water percentage (mass).