depression because depression arises from impurities within the lattice of a crystalized sample. We acquired a percent yield of 20.4%‚ which is relatively low. This result could be from part of the compound B solution being left behind in the Erlenmeyer flask when pouring the solution into the vacuum filtrate. The efficiency of a
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Lab 4. Volumetric Determination of Impure Sodium Carbonate (Na2CO3) Introduction: To determine the total amount of carbonate in unrefined sodium carbonate‚ soda ash‚ a titration is done using a standardized solution of HCl. Aqueous HCl is a strong acid and therefore almost completely disassociates into H+ and CL-. Therefore‚ when HCl is used in a titration‚ the H+ is the titrant. Carbonate in aqueous solution is able to accept a proton‚ i.e. it acts as a base. When carbonate accepts the H+ a bicarbonate
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Purpose Use a standardized potassium permanganate solution to analyze an unknown iron solution by using redox titration. Theory Reduction-oxidation titration is an analytical method based on electrons transferring between an oxidizing agent and a reducing agent in solutions. Chemical analysis can be built on Redox titration if four criteria are met: a) The reaction is completed in a thermodynamically spontaneous condition. b) The reaction is fast enough to give an operational result instantly
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Name: Shahid Hussain Subject: Chemistry Teacher: Dr Ramani Topic: Comparing Solutions Saturated Solutions | A solution that can hold no more of the solute at a particular temperature is said to be a saturated solution at that temperature. | When someone adds sugar to iced tea‚ the sugar disappears. If you add one teaspoon of sugar to iced tea‚ you get an unsaturated solution. If you keep
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the concentration of an unknown (acid or base) solution. 2. A solution of household vinegar (a mixture of acetic acid and water) is to be analyzed. A pipet is used to measure out 10.0 mL of the vinegar‚ which is placed in a 250-mL volumetric flask. Distilled water is added until the total volume of solution is 250 mL. A 25.0-mL portion of the diluted solution is measured out with a pipet and titrated with a standard solution of sodium hydroxide. The neutralization reaction is as follows:
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The Titration of a Basic Solution of Unknown Molarity with a Standard Hydrochloric Acid Solution Abstract The aim of the experiment was how to determine the molarity of a solution. My hypothesis was if I have to determine the molarity of a NaOH solution‚ then I would have to use a standard solution of HCl solution because I would need to neutralize each other to determine the concentration of the solution of NaOH. The method that I used for this experiment was titration. Titration helped
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Marie Alessandra T. Reyes Group 4 18L Quantitative Determination of the Acidity of Soft Drinks I. Introduction Soft drinks are well known beverages among the young that are consumed mostly for pleasure. These beverages normally contain flavoring‚ sweeteners coloring‚ carbonic acid and acids. Carbonic acid and acids play an important part in the formulation of soft drinks. They enhance the flavor and give a pleasant refreshing ’lift ’ to the drink. The type of acid used can even affect the palatability
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Aspirin Goggles were obtained and put on before entering the lab area. 2.0 grams of salicylic acid should be measured and placed into a 125 mL Erlenmeyer flask. 5.0 mL of acetic anhydride and 5 drops of 85% phosphoric acid was added to the Erlenmeyer flask. Drops of distilled water were added to rinse down bits of solids that were on inner wall of the flask. Mixture was heated on the hot plate for fifth-teen minutes‚ at 75 degrees Celsius. Two mL of distilled water was added 10 minutes into heating
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ethanol and 60% water) was added to another Erlenmeyer flask. Next‚ 0.10M of NaOH was filled up to the 0.00ml mark in two 50-ml burettes. Placing the flask containing solution 1 on the magnetic stirrer and clamp a burette containing 0.10M of NaOH above the flask. The two kinetic runs will be carried out one after another. A stir bar was placed into the flask containing solution #1 and 3-5 drops of phenolphthalein indicator solution to the reaction flask. To start the reaction‚ 4.91x10^-3 mol of alkyl
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Lab Report Iodination of Acetone Temperature as a Variable Objective The objective of this lab is to determine the energy of activation of the iodination of acetone. This will be done by performing the reaction at differing temperatures. The same reaction orders we obtained for the previous lab will be incorporated into this experiment. The equation Ea = -8.31 x slope of ln k vs. 1/T(K) will be used to determine the energy of activation required for this this reaction. Hypothesis
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