substances. In this technique‚ a solution is combined thoroughly with a second solvent that is immiscible with the first solvent. The solute is extracted from one solvent into the other because it is more soluble in the second solvent than in the first. In this experiment‚ there were two types of extraction used and these were the Liquid-liquid extraction and Solid-liquid extraction. Liquid-liquid extraction involves a liquid solvent to remove a liquid component from liquid while Solid-liquid extraction
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I. DISCUSSION: Differences between organic and inorganic compounds based on structure‚ type of bond and some common physical and chemical properties. II. PROCEDURE: A. SOLUBILITY 1. To 2 mL. each of the following solvents: water‚ ethyl alcohol and ether‚ add a pinch of benzoic acid and shake.
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within solute species oppose dissolving. Stronger forces between species favor dissolving. For molecular solutions‚ this can be summarized as “Like dissolves like.” In other words‚ solutes dissolve in solvents that have the same type of intermolecular forces. An immiscible solute and solvent are illustrated at right. Helium–oxygen mixtures are sometimes used as the breathing gas in deep-sea diving. At sea level (where the pressure is 1.0 atm)‚ the solubility of pure helium in blood is 0.94
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add into the evaporating dish then mass them together. 3. Set the evap. dish on the ring clamp and start the burner then find the perfect flame. 4. Wait a certain amount of time depending on how much solution you have for the solvent to evaporate. 5. After all the solvent is gone mass the evap. dish with the sodium inside it. 6. subtract the original mass of the evap. dish and you’ll find your mass of the sodium. Then you can set up your equation and find the molarity. Data Trial 1-
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ΔT1 = Kfm where Kf is a constant that depends on the specific solvent and m is the molality of the molecules or ions solute. Table 1 gives data for several common solvents. Table 1. Molal Freezing Point and Boiling Point Constants | Solvent | Formula | Freezing Point (°C) | Kf(°C/molal) | Boiling Point (°C) | Kb(°C/molal) | Water | H2O | 0.0 | 1.86 | 100.0 | 0.51 | Acetic acid | CH3COOH | 17.0 | 3.90 | 118.1 | 3.07 | Benzene | C6H6 | 5.5 | 4.90 | 80.2 | 2.53 | Chloroform | CHCl3 | –63
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properties: •Stabilization of core material. •Inert toward active ingredients. •Controlled release under specific conditions. •Film-forming‚ pliable‚ tasteless‚ stable. •Non-hygroscopic‚ no high viscosity‚ economical. •Soluble in an aqueous media or solvent‚ or melting. •The coating can be flexible‚ brittle‚ hard‚ thin etc. Microencapsulation (Cont.): Coating materials: Gums: Gum arabic‚ sodium alginate‚ carageenan. Carbohydrates: Starch‚ dextran‚ sucrose Celluloses: Carboxymethylcellulose
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prescribed in I.P. and U.S.P procedures. A UV absorption maximum of drug was found to be 244 nm (Fig. 4.1). An Infrared spectrum of the drug was concordant with the reference spectra (Fig.4.2 and Fig. 4.3). Solubility Profile of Ketoconazole different solvents indicated that the drug was freely soluble in methanol‚ methylene chloride and insoluble in water‚ ether and slightly soluble in PBS (pH 7.4)‚ dichloromethane and very slightly soluble in chloroform‚ alcohol etc. Partition coefficient of the drug
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LAB REPORT FOR EXPERIMENT #2: PURIFICATION OF ACETANILIDE BY RECRYSTALLIZATION Your name TA’s name Your Partner’s name Lab Section OBSERVATIONS: A. SELECTING A RECRYSTALLIZATION SOLVENT | |Solubility Test (cold) |Solubility Test (hot) | |Water |insoluble |soluble | |pet ether |insoluble
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part of the lab concentrates on how different factors influence the rate of SN1 reactions. The factors that will be examined are the leaving group‚ Br versus Cl-; the structure of the alkyl group‚ 3◦ versus 2◦; and the polarity of the solvent‚ 40 percent 2-propanol versus 60 percent 2-propanol. Discussion/Theory/Reaction Mechanisms SN2 Reaction Mechanism: This reaction takes place by an SN2 mechanism. The reaction must be carried out in a very acidic solution because the OH group
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predetermined amount of cyclohexane. Introduction: One of the key concepts in this experiment is the term freezing point depression. The definition of this phrase is that when a solute is dissolved into a solvent‚ their collective boiling point will be less than that of the original boiling point of the solvent. This incidentally leads to another important definition‚ the colligative properties of a solution. This means a particular set of characteristics that are unique to that solution. As the freezing
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