experiment was started with a clear solution of sodium benzoate and HCl was added to it‚ ultimately producing benzoic acid. First‚ .3395 g of sodium benzoate was weighed‚ then it was dissolved in water‚ causing it to disassociate into ions. Next‚ 3M of HCl were added drop wise to the solution until it reached a pH of 2‚ thus introducing the hydronium ion. This addition caused a white‚ solid benzoic acid to precipitate out of the solution. A vacuum filtration system was used to separate the solid from the
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the textbook says in regards to the history and uses of the chemicals that are being utilized in the experiment. Nothing elaborate – just the basic idea behind the reaction. Reaction (3 points) Reaction: sodium benzoate + hydrochloric acid ( benzoic acid + sodium chloride Amounts: 2.00 g 5.0 mL 3M + HCl → + NaCl ***Note that if there is no “reaction”
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effectively killing most yeasts‚ bacteria and fungi. Sodium benzoate is effective only in acidic conditions (pH < 3.6) making its use most prevalent in foods such as preserves‚ salad dressings (vinegar)‚ carbonated drinks (carbonic acid)‚ jams (citric acid)‚ fruit juices (citric acid)‚ and chinese food sauces. It is also found in alcohol-based mouthwash and silver polish. More recently‚ sodium benzoate has become apparent in many soft drinks‚ including Sprite‚ Fanta‚ Sunkist‚ Dr Pepper and Coke Zero. It
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Objectives 1. To separate a mixture of an acid and a neutral compound into its component by extraction. 2. To determine the melting point and the yield of the benzoic acid and the unknown sample. 3. To determine the unknown sample whether is is Trimethylmethanol or 1‚2‚4‚5-Tetrachlorobenzene. Introduction Extraction is a process of transferring a solute from one solvent to another. It is usually used to separate one or more components from a mixture. Diethyl ether‚ dichloromethane
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solution of an acidic and organic compound and purify its respective acidic product through the techniques of an acid base extraction‚ recrystallization‚ and use of Melt Temp (melting point range). The reaction of an unknown acid (3-chlorobenzoic acid) with diethyl and sodium hydroxide was observed‚ and the solution naturally separated into an aqueous and organic solution. The mixture of acid and organic solution was created and then separated through the Hirsch funnel into separate beakers of an aqueous
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Experiment 2: Acid- Base Extraction Separation of an Organic Acid‚ a Base and a Neutral Compound Introduction: The extraction technique is often used in the organic lab to separate organic compounds from mixtures. One type of an extraction technique is the acid-base extraction‚ which is used to separate organic compounds from a mixture based on their acid-base properties.1 There are certain principles that must be taken into account when choosing a solvent system to perform an extraction. The solvents
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Unit 4B Task 2 Title Recrystallization of benzoic Acid Aim Equipment 1. Erlenmeyer flask 2. Graduated cylinder 3. Hot plate 4. Small beaker 5. Ice bath (if necessary) 6. Filter paper 7. Buchner funnel 8. Spatula 9. Weighing machine Method 1. Weighing paper was used to weigh approximately 1.00g of ‘impure Benzoic acid to produce re crystallization’. 2. Moved it to a 125ml Erlenmeyer flask. 3. Poured approximately 20ml of distilled water by using a graduated cylinder
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The obtained mass of benzocaine and benzoic acid mixture was measured to be 2.075 grams. Following being dried for a week the mass of benzocaine was recorded to be 0.250 grams‚ and benzoic acid was recorded to be 0.600 grams. The melting point range of benzocaine was measured to be 89.5°C-91.5°C‚ while benzoic acid’s melting point range was measured to be 129°C-131.3°C. The percent mass recovered was calculated to be 40.96% for the experiment. Table 1 illustrates the collected information. Starting
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benzoate .210 ml Cold water 1 ml 3 ml conical vial + Methyl benzoate 20.321 g Ice-cold methanol .3 ml Methyl benzoate 0.4095 g Crude product 0.6981 g Sulfuric acid (1st added) .50 ml Melting point (Literature value) 78-80 °C Sulfuric acid (2nd added) .15 ml Melting point (experimental value) 72.4-733.7 °C Nitric acid .15 ml Molar mass of methyl benzoate 136.15 g/mol Molar mass of methyl m-nitrobenzoate 181.15 g/mol Molar mass of HNO3 63.01 g/mol Melting point (Literature
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from willow bark – willow bark contain an active ingredient know as salicylic acid which used to make aspirin (pain reliever) Identifying salicylic acid Three chemical tests which are used to predict the structure of salicylic acid 1. Salicylic acid in aqueous solution is weakly acidic ( presence of COOH group) 2. Salicylic acid reacts with alcohols to form esters which give of strong odours. 3. When salicylic acid is added to a neutral solution such as iron chloride it turns intense pink colour
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