Conductimetric Titration and Gravimetric Determination of a Precipitate Objective: * Measure the conductivity of the reaction between sulfuric acid and barium hydroxide * use conductivity values to determine equivalence point * measure mass of a product to determine equivalence point gravimetrically * calculate molar concentration of barium hydroxide solution Procedure: * First‚ combine 10.0 mL of the Ba(OH)2 solution with 50 mL of distilled water. Then‚ measure out 60 mL
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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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sulfate in coal‚ which is the basis for this experiment. In any precipitation gravimetric analysis‚ the species to be determined is reacted with a reagent to yield a product that is: a) of known composition‚ b) is relatively pure‚ and c) of low solubility. Knowing the mass of the dried product and the mass of the original sample and their formula weights (to create a gravimetric factor)‚ the percent of the species to be determined can be calculated. In the analysis for sulfate‚ the sample to
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Biochemistry Exam I Terminology Boiling point is the temperature at which the vapor pressure of the liquid equals the pressure surrounding the liquid. At this temperature the liquid phase changes into the gaseous phase (also a colligative property) Melting point is the temperature at which the solid and liquid phases are in equilibrium. At this temperature the solid state changes into a liquid phase (also a colligative property) Specific heat is the amount of energy (in joules or calories) needed
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Separation of the Components of a Mixture General Chemistry 1 (Chem 101)‚ ISP SCUHS Report 2 January 26‚ 2014 Abstract The analyses of mixture were to distinguish and identify homogeneous mixture by using the techniques of decantation and sublimation. By performing these techniques‚ we examined our solutions such as SiO2 (sand)‚ NH4Cl (ammonium chloride)‚ and NaCl (sodium chloride) and mixed H2O (water) with each solution after being heated. After examining our solutions‚ we made calculations
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Date of experiment: September 3rd‚ 2013 Organic Chemistry II – CHLB330 Name: Symone MoxeyLab Partner: Lynden Cooper Isolation of caffeine from tea leave Abstract:- Introduction:- Caffeine is probably the most commonly used addictive drug. This drug is found in a number of things ingested by people. It belongs to a group of nitrogen bases called purines. Because caffeine possesses these base-like properties‚ it is described as an alkaloid. They usually taste bitter and often are physiologically
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advantage of the different physical and chemical properties. Such as; different boiling points‚ melting points and their solubility properties. To do this a chemist can also asses the differences between acidic and basic substances when they are added to water soluble mixtures. Within this current experiment I will asses the pharmaceutical preparation of Panacetin‚ by using it ’s solubility along with other organic molecules. We know that Panacetin is made up of sucrose‚ aspirin and some other unknown
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another solvent. Acid-alkaline extraction is a commonly used method to recover a compound from solid or liquid and also a form of solvent-solvent extraction. Acid-alkaline extraction is a method to separate compounds according to their relative solubility in two different immiscible solutions. Usually‚ acid-alkaline extraction is being used to recover a compound from solid or liquid. The two solvents used to conduct acid-alkaline extraction must be insoluble to one another. Therefore‚ the mixture
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NR Cloudy Almost White Cloudy Almost White Cloudy White Ni(NO3)2 Cloudy Mint Green NR NR NR Hazy Clear Liquid Hazy Clear Liquid Cloudy with almost a mint green color QUESTIONS (10 points) 1. Compare your results with the solubility rules. Do your results generally agree with them? Yes‚ I feel like my results were comparable to the rules on the table in the chemistry text. 2. Why is water a good solvent for ionic substances? Water is a great solvent because it has an uneven
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Objective: To test the ten compounds found in the physical data table that follows‚ and observe them by categorizing the reactions as Sn1 and SN2. Physical data: Compound M.W. (g/mol) Melting Point (C°) Boiling Point (C°) Density (g/mL) Solubility Safety Considerations 2-chlorobutane 92.57 -140 68 0.87 very slightly soluble in cold water Irritant with skin‚ lung‚ and eyes. 2-bromobutane 137.03 -112 91.2 1.25 Irritant with skin‚ lung‚ and eyes. 1-chlorobutane 92.57 -123 79 0.88 insoluble
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