Separating the components of the Panacetin using Extraction and Evaporation Objectives: The purpose of this experiment was to perform the separation of aspirin‚ sucrose and an unknown analgesic‚ which are constituents of Panacetin using the methods of filtration‚ extraction‚ and purification Structures: Sucrose Unknown Aspirin Table of Reagents and Solvents: Substance MW Wt. or Vol. Moles MP or BP‚ ºC Density g/mL Hazards Panacetin na 2.014 g na na na Harmful if swallowed
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crystallize first As the crystals are formed‚ the correct molecules that will fit in the crystal lattice are selected while the wrong molecules are ignored‚ resulting in a pure solid - Depends on: 1) solubility of the compound 2) differences in solubility of the desired solutes & impurities dissolved in the solvent - Common Solvents Used: Solvent | Formula | Polarity | Boiling Pt. (oC) | Water | H2O | Very Polar | 100 | Ethanol | CH3CH2OH | Polar | 78
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EXPERIMENT NO. 9 CHEMICAL EQUILIBRIUM Audrey De Castro FCD3‚ Group 9‚ Ms. Sarah Sibug Kristine Tavares March 27‚ 2014 I. ABSTRACT Chemical equilibrium is mostly involved in industrial processes such as synthesis
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Chapter 11: Measuring solubility Measuring Solubility Solubility: the maximum amount of that substance that can be dissolved in a that temperature Saturated solution: a solution which no more solute can be dissolved at that temperature Measuring solubility Determine the maximum mass of solute that can be dissolved in 100 grams of solvent at a particular temperature Worked Example A maximum of a 6g of solute can be dissolved in 20g of water at 20ºC. What is the solubility of this solute in water
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deductive thought process. Qualitative analysis of cations requires an extensive knowledge of various aspects of chemistry including acid-base equilibria‚ complex ion equilibria‚ solubility‚ etc. However‚ in the deductive process‚ common sense and logic can be as helpful as a knowledge of the chemistry involved. In this lab you will be working with a solution containing a mixture of cations. Before individual components of the mixture can be successfully identified‚ they have to be separated. The
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-12:15 PM Room 113 MRB (CRN 10304)--Cole Lecture Section 001: Tuesday/Thursday 1:00-2:15 PM Room G24 EIE (CRN 10305)--Cole Lab Section 002: Wednesday 10:30 – 11:20 AM Room 421 ARM (CRN 14335)— Cole Lab Section 003: Wednesday 11:30 AM – 12:20 PM Room 421 ARM (CRN 14336)— Cole Lab Section 004: Wednesday 12:30 – 1:20 PM Room 421 ARM (CRN 14337)— Cole Lab Section 005: Wednesday 1:30 – 2:20 PM Room 421 ARM (CRN 14338)—Cole Important Things You Should Know About This Course: 1
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Experiment 1: Mixtures Aim: To develop an understanding of different types of mixtures including solutions and examine the different solubilities of some solutes and two solvents: water and ethanol Equipment Bunsen burner Tripod Gauze mat Beakers (2 x 100mL) Boiling chips Distilled water Sodium chloride Sodium chloride (solid) Glass rod Measuring cylinder (25mL) Ethanol Watch glass Thermometer 100% Orange Juice 100% Apple Juice 100% Prune Juice Solder Fruit Scone Charcoal Copper(II) Chloride Magnifying
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PROCEDURE A. Effect of temperature on solubility of a solid in water. a. Put 1g of KCl (Potassium Chloride) in 10 ml water with an ignition tube at 10°C‚ then shake and observe the solubility of KCl. b. Heat the solution to 40°C and not higher‚ then stir and observe its solubility. c. Add another gram of KCl in the mixture‚ then stir and observe the solubility. Heat the mixture in an 80°C water bath then shake and‚ once more‚ observe the solubility of the KCl. d. Repeat the procedure with
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there are any impurities that have the same solubility as the main component‚ then a different solvent needs to be chosen.) When organic substances are synthesized in the laboratory or isolated from plants‚ they will obviously contain impurities. Several techniques for purifying these compounds have been developed. The most basic of these techniques for the purification of organic solids is recrystallization‚ which relies on the different solubilities of solutes in a solvent. Compounds‚ which are
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Abstract: The objective of this lab is to calculate the theoretical‚ actual‚ and percent yield of the product from a precipitation reaction. It is also to learn concepts of solubility and the formation of a precipitate. The Experiment and Observation: Weigh out your 1.0g of CaCl2-2H20 and put it into the 100mL beaker‚ add your 25mL of distilled water and stir to form the calcium chloride solution. Next‚ use stoichiometry to determine how much Na2CO3 and put it into a small paper cup. Then add
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