MATERIALS AND METHODS: Before the acetic acid solution could be titrated with sodium hydroxide (NaOH), the actual concentration of NaOH needed to be determined. By way of standardization, the actual concentration of NaOH was established, to account for the fact that the solid is not pure and for its tendency to react with carbon dioxide in the air. A 50 mL burette (±0.01 mL, Kimax) was rinsed thoroughly, twice with reverse osmosis water, and then twice with approximately 5 mL of ~0.25 M NaOH solution
BIOC 2200 – Experiment 1: Buffers and the effect on amino acids Aiden Forsyth 1009696399 Wednesday PM Bench 13 Results Questions A1. By the Henderson-Hasselbalch equation (Plumber, 2004). pH=pka+log〖([HA])/([A^-])〗 n_([HA])=M*V=0.10 mol/L*0.050L=0.0050 mol n_[A^- ] =n_NaOH=M*V=0.20 mol/L*0.001L=0.0002 mol Since acetic acid is transformed to sodium acetate there is a consumption of [HA] by the amount of moles of sodium hydroxide. pH=4.76+log〖0.0002/(0.0050-0
Sodium Hydrogen Carbonate and Acetic Acid Reaction Introduction Not knowing whether calculations on a paper or an experiment are conducted correctly is one of the problems faced in chemistry. Luckily to ensure both calculations are correct, getting a one hundred percent yield is a necessity. “The actual yield of a product as a percentage of theoretical yield,”1 is how to determine the percent yield of a reaction. Actual yield is the amount, in grams, that a reaction actually produces while theoretical
it is clear that neither classical thermal pasteurization nor sterilization, nor microfiltration were sufficient to obtain a shelf-stable product without additives. Efficient results were obtained by adding molecules such as nisin, ascorbic acid or citric acid and sodium metabisulphite.
Purpose: To create sweet smells from putrid acids by following a formal laboratory procedure. Hypothesis: If carboxylic acids and alcohols perform chemical synthesis, the resulting product will smell sweet. Materials: 50 ML beaker Hot plate 3 microscale test tubes Boiling stones 3 plastic pipettes Scissors to cut pipettes Pencil or marker Organic acids and alcohols Procedure: 1. A 50 ML beaker was filled with around 30 ML of water. 2. A boiling stone was dropped in. 3. The beaker
The Knorr synthesis of the pyrrole, 2,4-diethoxycarbonyl-3,5-dimethylpyrrole, was achieved using an α-amino ketone, ethyl acetoaminoacetate and reacting it with its predecesso r, ethyl acetoacetate in a double condensation reaction . The product was analysed by 1H NMR, 13C NMR, mass spectrometry and IR spectroscopy giving positive results . Introduction Pyrrole has been a molecule of great interest due to its heterocyclic aromatic properties. The lone pair on the nitrogen is delocalised within
milk are largely water-soluble due to amine and carboxylic acid side chains, amine’s are protonated, and thus positively charged, at a pH near that of 7.44 or human physiological pH2. Amine’s remain unprotonated at high pH2. Carboxylic acids, however, are protonated at low pH and unprotonated at higher pH, such as physiological pH2. Carboxylic acids retain a negative charge in their unprotonated state, at physiological pH carboxylic acids are negatively charged side chains. While the protein retains
In this experiment, luminol was synthesized and investigated the chemiluminescence reaction. The starting material, 5-nitro-2,3-dihydrophtalazine, was added by reagents, refluxed and vacuum filtered to get luminol. Using stock solutions, we mixed our luminol product with sodium hydroxide, hydrogen peroxide and potassium ferricyanide in a dark room to observe a blue light. In the end there was a 121% yield of luminol and experienced a blue glow. Introduction Luminol is an organic compound that is
glass, fume hood, 10 mL and 50 mL graduated cylinder. To synthesize aspirin a boiling-water bath was prepared by adding 300-mL tap water to the 600-mL beaker and placed on a hot plate with a ring stand around the beaker. Then 2.1g of salicylic acid, 4-mL acetic anhydride, and 5 drops of concentrated H2SO4 solution were added to the Erlenmeyer flask and the flask was swirled gently until some of the solids dissolved and some undissolved. Utilizing the clamp, the Erlenmeyer flask was placed inside
water and 1 ml conc. HCl and boil for 10 minutes. In this way the unchanged starting materials and the basic zinc salt are dissolved. Separate the fluorescein from the aqueous liquid by filtration, wash with water until the filtrate is no longer acid. Dissolve a particle of the preparation in a little ammonia and dilute in a beaker with one liter of water. Determine the weight and melting point of the solid. Calculate the % yield of the product. Obtain and interpret an infrared spectrum of
...oncentration as it may have generated the greatest concentration of tartaric acid, whereas Wines B and C may have produced other acids present in wine, such as malic, lactic, citric, acetic or succinic acid. Esters are compounds formed by condensation between an acid and an alcohol. In the Investigation, ethanol in the wine would have provided the alcohol and the acids present would have produced the acid component, therefore it was predicted that the taste test would see to the detection
this? What kinds of bond will form, and will the old bonds break? Baking soda is a solid, or you can say white crystals. It is known as a type of salt, and it is soluble. Baking soda is made out of carbonic acid too. The chemical formula for baking soda is NaHCO3. Vinegar contains acetic acid and water. It is a type of liquid. The chemical formula for vinegar is CH3COOH. If I'm going to mix vinegar and baking soda together, will it be a mixture or a compound? Now, vinegar will be the solvent because
acetylsalicyclic acid in one commercial aspirin tablet, using the principle of back titration. (II) Discussion Back titration rather than direct titration was used because there was no suitable indicator for acetylsalicyclic acid and sodium hydroxide solution. Therefore, excess amount of NaOH was used to react with acetylsalicyclic acid. The number of moles of unreacted NaOH was determined from titration with hydrochloric acid. Eventually the number of moles of acetylsalicyclic acid and its percentage
Question 1 is, Vinegar is made of acetic acid and water. Explain how it was able to remove the calcium shell. My answer was, the acetic acid broke down the shell. Question 2 is, What happened to the size of the egg after remaining in vinegar? My answer was, After remaining in vinegar the egg got bigger. Question 3 is, Was there more or
hoods. Sulfuric acid can cause burns if it comes in contact with skin. If contact with skin does occur wash the area with 5% sodium bicarbonate solution. The basic solution if in contact with skin rinse the area with 1% acetic acid solution (1). Acid catalyzed hydration of alkenes produces and alcohol by the addition of water through carbon-carbon π-bonds. In other terms this reaction is the reverse of acid catalyzed dehydration which removes an alcohol. The mechanism for acid catalyzed hydration
The Knorr Synthesis of Pyrroles Experimental A mixture of ethyl acetoacetate 1 (7.52 g, 7.5 mL) in glacial acetic acid (18 mL) was prepared and cooled to 5oC while stirring. Sodium nitrate solution (2.1 g in 5 mL deionised water) was added at such a rate that the temperature of reaction did not exceed 7oC. Once this addition was complete the mixture was stirred with cooling for 10 minutes before being allowed to warm to room temperature. Zinc dust (4.0 g) was added to the reaction mixture in
determined to be Test 3: Pressure Analysis. While it was not as effective as Test 1: Solution Conductivity when adhering to principles of Green Chemistry, but Test 3 provided the most accurate results. The reactions between Na2CO3 or NaHCO3 and Acetic Acid produced Sodium Acetate, Water and Carbon Dioxide. While it did produce CO2 and Sodium Acetate which are waste products, they are considered non-hazardous being the side products of the common baking soda and vinegar reaction. Test 2, Thermal Decomposition
containing cooking oil did show signs of corrosion it was only because it was in the presence of water. Furthermore, water is a corrosive agent and ultimately, the hypothesis was proven correct. References: "Rusting Out: How Acids Affect the Rate of Corrosion." Rusting Out: How Acids Affect the Rate of Corrosion. N.p., n.d. Web. 20 May 2014. . "Sodium Bicarbonate and Metal." Sodium Bicarbonate and Metal. N.p., n.d. Web. 20 May 2014. . "What is Corrosion?." About.com Metals. N.p., n.d. Web. 20 May 2014
esterification reaction was observed. A Fischer esterification is a reaction that converts a carboxylic acid into an ester. Within the reaction, the hydroxyl portion, -OH, of the carboxylic acid is replaced by an -OR group. The byproduct is water which is also a nucleophile. Therefore, water can be added back into the compound and undergo hydrolysis on the newly formed ester which produces the starting carboxylic acid. To make sure the reversibility did not occur, the reaction mixture was heated to force the
The purpose of this experiment is to examine the reactivity of different compounds. To accomplish this, different types of benzene (aniline, acetanilide, phenol, or anisole) will be brominated. The reactivity and activation strength will determine of the compound is polyhalogenated, or monohalogenated. In this experiment it is to be predicted in which order the reaction substitution(s) will occur and the reactivity order of each of the benzene compounds. The product will then be analyzed and