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 of 0.100
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sulphate is determined quantitatively as barium sulphate by gravimetric analysis. This determination consists of slowly adding a dilute solution of barium chloride to a hot‚ unknown sulphate solution which is slightly acidified with concentrated hydrochloric acid. A white precipitate will formed and is then filtered off‚ washed with deionised water‚ dried in the oven and weighed as barium sulphate. The percentage of sulphate is calculated from the weight of barium sulphate. (B) Objective The purpose
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color of the flame. In this experiment‚ unknown solution #1 was proven to contain lead (Pb2+) and barium
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This experiment contains three separate procedures in which Aluminum Potassium Sulfate(Alum) will be melted‚ massed out and mixed with Barium Nitrate‚ along with distilled Water. Procedure one we completed two trials of melting two separate 0.01g of Alum and making a comparison to the literature temperature of 92.5‚ to do this we attached an Alum filled capillary tube to a thermometer and inside a beaker placed over a Bunsen burner. Procedure two consisted of placing 2.00 grams of Alum into a crucible
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written about determining the quantitative amount of sulphate inside barium sulphate‚ BaSO₄‚ using the method of gravimetric analysis. This quantitative determination is done by the addition of a dilute solution of barium chloride slowly to a hot unknown sulfate solution slightly acidified by concentrated hydrochloric acid‚ HCl. The white precipitate of barium sulphate is filtered off‚ washed with water‚ oven-dried‚ and weighed as barium sulphate. The quantitative amount of sulphate is deduced from mathematical
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CHAPTER I INTRODUCTION The appendix is a closed-ended‚ narrow tube that attaches to the cecum (the first part of the colon) like a worm. (The anatomical name for the appendix‚ vermiform appendix‚ means worm-like appendage.) The inner lining of the appendix produces a small amount of mucus that flows through the appendix and into the cecum. The wall of the appendix contains lymphatic tissue that is part of the immune system for making antibodies. Like the rest of the colon‚ the wall of the
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APPENDICITIS is a condition characterized by inflammation of the appendix. It is classified as a medical emergency and many cases require removal of the inflamed appendix‚ either by laparotomy or laparoscopy. Untreated‚ mortality is high‚ mainly because of the risk of rupture leading to peritonitis and shock.[1] Reginald Fitz first described acute and chronic appendicitis in 1886‚[2] and it has been recognized as one of the most common causes of severe acute abdominal pain worldwide. A correctly
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The sulfate is precipitated as barium sulfate from a solution containing a known mass of fertiliser by adding from a solution containing a known mass of the fertiliser by adding an excess of barium chloride solution: The proportion of sulfate ions and therefore of sulfate in the fertiliser is determined by collecting and weighing the precipitate that is formed
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Analysis of Alum The objective of this lab is to run tests on a compound and analyze the substance itself‚ and then determine whether or not the compound is actually alum. Jill Cline Period 3 November 19‚ 2013 Laurel Hergenroeder and Sarinah Martelli Introduction/Purpose The purpose of this experiment is to run various tests on the substance called alum. (AlK(SO4)2 ∙ 12H2O). These tests like the process of filtration heating the solution will reveal things
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Superconductivity Jaron Hartman In collaboration with Stefan Eccles Senior Lab Abstract: Superconductivity is the phenomena of a material to have an electrical resistance of zero when cooled to a certain temperature known as the critical temperature. The phenomenon of superconductivity was first observed in 1911 by Heike Kamerlingh Onnes when cooling mercury down to a temperature of 4.2 K. Since then‚ many advances in the field of superconductivity have been made. In 1986‚ superconductivity
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