Chemistry Location and Date II. Abstract The aim in this lab was to determine the empirical formula of an oxide of magnesium through combustion in air. This was achieved by heating an established mass of magnesium in air inside of a crucible‚ ultimately attaining a compound that contained Mg and O. The major result of the experiment was the empirical formula of the oxide of magnesium. III. Introduction An empirical formula is defined as a formula that gives the simplest ratio of the relative number
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Lead (II) nitrate and potassium iodide solutions 6. Pour about 2.0 mL of lead (II) nitrate into the test tube. Add 5 to 10 drops of potassium iodide solution to the test tube and record your observations of the reaction. 7. 8. 9. Magnesium metal and hydrochloric acid solution 10. Place one scoop of magnesium turnings into the test tube. Add hydrochloric acid slowly and observe the reaction. Next‚ place a burning splint near the mouth of the test tube to test for the presence of hydrogen gas. 11. 12. 13. Electrolysis of water
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magnesia was invented in 1817 by the Irish pharmacist Sir James Murray (1788–1871). Murray built a plant to produce a mixture of magnesium hydroxide in water that he sold for the treatment of a variety of disorders‚ including heartburn‚ stomach acidity‚ bladder and bowel problems‚ and "female problems." He said that the liquid mixture was much more effective than powdery magnesium hydroxide which had previously been used for the same purposes. In 1880‚ New York chemist Charles Henry Phillips (1820–1882)
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Unit 3 – Virtual Labs Letizia Schianodicola Lab #1 – Atomic Weight of Magnesium 1. Moles of hydrogen evolved‚ from chemical property dialog for beaker: a. 0.000411 mol H2 2. Calculate the atomic weight of Magnesium. Atomic weight of Mg = weight of Magnesium/moles of H2. b. 59‚136.253 g/mol Mg (24.305 - weight of Mg / 0.000411 mol H2) 3. Calculate the # of molecules of H2 that were produced in the reaction – use Avagadro’s number –
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* Assorted measuring cylinders * Stopwatch * Thermometer * 0.1g of magnesium powder * 10cm3 of sulphuric acid Method: First‚ I will measure the correct amount of magnesium I need‚ which is 0.1g. Then I will measure out 10cm3 of the sulphuric acid into the measuring cylinder. Next‚ before I start the experiment‚ I will measure the starting temperature of the acid. Then I will place the magnesium and sulphuric acid in a beaker. I will measure the temperature every twenty seconds
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Semester – CH 2307 TECHNICAL ANALYSIS LAB -2010 INDEX SHEET CYCLE ONE Date of Condn. Date of Subn. Sign 1 Estimation of COD of the given sample of water. 2 Estimation of Manganese in the given pyrolusite ore. 3 Estimation of Magnesium by EDTA method. 4 Estimation of purity of drug using pH meter. 5 Estimation of Ammonia in ammonium salts. 6 Polarimetric estimation of sugar CYCLE TWO Date of Condn. Date of Subn. Sign 7 Estimation of Phosphorous
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UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS International General Certificate of Secondary Education CHEMISTRY Paper 1 Multiple Choice Additional Materials: Multiple Choice Answer Sheet Soft clean eraser Soft pencil (type B or HB is recommended) 0620/01 October/November 2008 45 Minutes *6400528663* READ THESE INSTRUCTIONS FIRST Write in soft pencil. Do not use staples‚ paper clips‚ highlighters‚ glue or correction fluid. Write your name‚ Centre number and candidate number on the
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Chung-Harris and Mike Taylor Chemistry for CAPE by Susan Maraj and Arnold Samai Periodic Trends in Group II Elements in Group II The elements in Group II are called alkaline earth metals. Be‚ Mg‚ Ca‚ Sr‚ Ba‚ Ra Beryllium‚ Magnesium‚ Calcium‚ Strontium‚ Barium‚ Radium These elements bond by metallic bonds (intramolecular forces) to form giant metallic structures. The size of the atoms increases down the group Physical properties of Group II metals Ionization
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for the following compounds that contain polyatomic ions. (a) Sodium hydroxide NaOH (b) Potassium nitrate KNO3 (c) Magnesium sulfate MgSO4 (d) Aluminum phosphate AlPO4 (e) Aluminum nitrate Al(NO3)3 (f) Ammonium nitrate NH4NO3 25. Name each of the following binary ionic compounds. (a) NaBr sodium bromide (b) MgS magnesium sulfide (c) CaO calcium oxide (d) MgCl2 magnesium chloride (e) AlF3 aluminum fluoride (f) CaI2 calcium iodide 26. Name each of the following binary molecular compounds
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essential to human dietary needs. c. To facilitate the secondary use of the desalinated water‚ for example‚ irrigation. Dosages of 60 to 120 mg/L as CaCO3 of calcium containing chemicals like lime‚ calcite‚ calcium‚ hypochlorite‚ or calcium and magnesium containing chemicals like dolomite are added to the desalinated water. this is important for the water distribution
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