Chemicals Sample Structure Purpose Physical Properties Hazards Salicylic Acid Starting Material Appearance: white powder Molar Mass: 138.12 g/mol Melting Point: 1590C Boiling Point: 2110C Density: 1.44 g/cm3 Mildly irritating (pulmonary irritants). Harmful by inhalation‚ ingestion and through skin absorption. Acetic Anhydride Starting‚ Material‚ serves also as the solvent colorless liquid with a smell of acetic acid Molar Mass: 102.09 g/mol Melting Point: -73.1 0C Boiling Point:
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Experiment #1: Synthesis of Salicylic Acid From Wintergreen Oil By: Asad Razzaq TA: Date: 18/01/2015 222/Lab Section 8 Introduction Salicylic acid‚ used in production of substances used worldwide such as commonly used analgesic drug aspirin(cite)‚ can be obtained from natural resources such as wintergreen oil or can be synthesized. Through a series of chemical reactions with cheap raw materials beginning with beginning with methyl salicylate and‚ it is a cheaper and more
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etc. Synthesis of Aspirin and Methyl Salicylate. The two compounds we will be preparing‚ aspirin (acetylsalicylic acid) and oil of wintergreen (methyl salicylate)‚ are both organic esters. An ester is a compound that is formed when an acid (containing the COOH group) reacts with an alcohol (a compound containing an -OH group). O C R1 O H O + H O C R2 R1 O R2 + H O H acid alcohol ester water Here R1 and R 2 represent groups such as CH3 - or CH3 CH2 -. The reaction type shown
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Formation of ester from carboxylic acid. MECHANISM: When the carboxylic acid is treated along with the acid catalyst and alcohol[R-OH]‚ It gives rise to the formation of ester along with water. Furthermore alcohol is used in an excess amount in the reaction‚ because this reaction is probably in equilibrium. Whereas alcohol is employed as a solvent‚ so it is used quiet larger in the reaction mechanism. Various other acids can also be used as the solvent
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from salicylic acid and acetic anhydride. Those two chemicals are mixed together along with sulfuric acid to form a crude solid. Filtration is used separate the impurities from the crude aspirin. To get purified aspirin‚ the precipitate was heated until all the excess had been removed. The end product is pure dry aspirin. Though there was too much room for error the yield percentage will almost never be a hundred percent. INTRODUCTION: In 1897 Felix Hoffman synthesized acetylsalicylic acid when
Free Aspirin Acetic acid Carboxylic acid
SYNTHESIS OF THE PHARMACEUTICAL ASPIRIN (ACETYLSALICYLIC ACID) AIM: The aim for this experiment was to synthesise a small amount of aspirin with salicylic acid as the starting product and sulphuric acid as the catalyst. The product obtained from this reaction will be impure and will need to be purified. This will be done by recrystallization. We will then record the products’ melting point and calculate the yield in order to determine the degree of purity of the aspirin sample. Diagrammatic scheme
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acetylsalicylic acid‚ was synthesized from salicylic acid and acetic anhydride. In the reaction the hydroxyl group on the benzene ring in salicylic acid reacted with acetic anhydride to form an ester functional group. This method of forming acetylsalicylic acid is an esterification reaction. Since this esterification reaction is not spontaneous‚ sulfuric acid was used as a catalyst to initiate the reaction. After the reaction was complete some unreacted acetic anhydride and salicylic acid was still be
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group. This new product is salicylic acid. Acetic anhydride is added to the salicylic acid to add an acetyl group to carbon 2 which will create acetylsalicylic acid
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Aspirin Background Aspirin Aspirin‚ or acetylsalicylic acid (ASA) is a salicylate drug‚ and is generally used as an analgesic (something that relieves pain without producing anaesthesia or loss of consciousness) for minor aches and pains‚ to reduce fever (an antipyretic)‚ and also as an anti-inflammatory drug. Aspirin works by prohibiting biological substances such as prostaglandins. Many different prostaglandins exist in the human body each serving a plethora of physical functions.
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The full strength 1M HCl acid had a pH level of 3.12 (Table 3.1). Sample A2 to A4 remained in the pH 3 level‚ while sample A5 and A6 had a pH range of 4 (Table 3.1). The pH level for 1M HCl dilutions slightly increased between each sample (Table 3.1). The diluted solutions of 1 M NaOH showed a few unexpected results. The original solution of 1 M NaOH was at a pH level of 11.50 (Table 3.1). However‚ the pH of sample B2 increased to 12.81 (Table 3.1). The remaining samples had a decreasing pH pattern
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