02 4/02/2013 Abstract A sample of soil was tested for possible contaminants and other information using a variety of techniques including moisture analysis‚ pH measurement‚ acid-base titration‚ chloride-ion electrode analysis‚ and flame testing. The sample had a greater concentration of chloride ions‚ no measurable CaCo3 ‚ and lower than standard moisture content. It was contaminated with KCl and likely HCl ionic solids. Introduction Soil is a vital component of any environmental network
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of chlorine ions Aim: To compare the concentration of chloride ions in pool and tap water respectively. Background: Tap water contains a variety of dissolved ions such as Ca2+‚ Mg2+‚ Na+‚ HCO3- and Cl-. In this experiment we will determine the concentration of the Cl- ions‚ and comparing it to the concentration found in a sample of pool water. The method used is the standard one for determining the concentration of chloride ions: titration with silver nitrate solution of known concentration
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Barium chloride Calcium chloride Copper (II) chloride Magnesium chloride Potassium chloride Sodium chloride Unknown solids containing a single cation and labelled X‚ Y and Z Apparatus: Bunsen burner Insulation mat Platinum wire (or Nichrome wire)‚ Watch glass Safety precaution: As concentrated hydrochloric acid is corrosive‚ skin contact should be avoided. It is preferable to use polythene gloves and wear goggles while handling it. Copper (II) chloride and barium chloride are highly
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Gravimetric Analysis of a Chloride Salt CHEM 1001 Purpose: To illustrate typical techniques used in gravimetric analysis by determining quantitatively the chloride content in an unknown soluble salt. Theory: AgCl(s) is a very insoluble solid‚ yet still does have some solubility. Because of these traits‚ the following reaction is able to occur: Ag+(aq) + Cl−(aq) → AgCl(s) . This reaction is able to occur in both directions. When a soluble silver salt such as AgNO3 is added to a solution containing
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is directly related to the solubility of iodine in water in this case. 2. Ammonium chloride will be more soluble in hot water as in an endothermic reaction‚ increasing the temperature (which is the same as adding heat - one of the reactants) will cause the position of equilibrium to shift towards the products to compensate for the change. More products are a result of increased solubility of Ammonium Chloride with water when temperature is increased. Post Lab Questions 1. CoCl42- ions are
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Complete report available @ http://www.rnrmarketresearch.com/hot-melt-adhesives-market-by-products-eva-styrenic-block-polyolefin-polyurethane-others-by-applications-packaging-non-woven-pressure-sensitive-construction-bookbinding-others-by-geo-market-report.html Hot Melt Adhesives Market are defined as adhesives that melt and flow on application of heat and solidifies on cooling to give a strong adhesion. HMA are 100% thermoplastic solids at temperatures below 80°C. They are applied in a molten
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Diary Recount - Received design brief and folio assignment for breadbox. - Received long piece of timber for 12 slats and cut each to 350mm long. - Jackplaned dozen slats to10mm thick and chamfered each to 3mm. - Marked rebate joints on top and cut with electric router and jig. - Marked curve on both sides of breadbox with pencil and template. - Nailed sides together with 40mm bullet-head nails and Warrington hammer followed line with jigsaw - Sanded sides evenly with disc sander. Finished
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Chemical Equilibrium: Le Châtelier’s Principle Abstract This experiment entitled "Chemical Equilibrium" aims to help students to investigate the effects of concentration and temperature upon the position of equilibrium in a cobalt chloride solution‚ Co(H2O)62+. In this experiment‚ cobalt crystal is dissolved with distilled water and ethanol which the initial colour is purple-pinkish and a few drops of concentration of HCl is added to the test tube‚ the final colour is in deep blue colour. Upon
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Experiment 2 – Identification of Inorganic Solids Jesse Galina CHM 101 Lab Monday October 1‚ 2012 Unknown Solid – 2 Identifying my cation was rather easy because of the color of the powder when it was first given to me. It was pinkish/slight red when solid and when it was grounded up even further. This observation ruled out every cation except for some hydrated Co (II) salts. After being dissolved in water‚ the solution turned pink which agrees with the statement that the cation was Co
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Synthesis Procedure 1 -1.0 Introduction A Cobalt-Amine-Halide compound is synthesized from cobalt (II) chloride hexahydrate. An orange-tinted solid is produced and is considered to be unknown since the specific ligand amounts are unknown. By determining the percent composition of various elements and compounds in the unknown‚ its true identity can be predicted. Chloride‚ ammonia‚ and cobalt are three examples of percent compositions determined to help narrow the selection of possible unknowns
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