Locker# 1137 Date of Experiment: May 11‚ 2014 Date of Submission: May 16‚ 2014 Purpose: To determine the identity of an unknown hydrated salt calculating the percent water loss after heating and also to determine the empirical formula of magnesium oxide. Results: Table 1: Determination of the mass of waters of hydration of an unknown hydrated compound. Hydrated Compound code: C-14 Mass (g) Crucible + Lid 30.581g Crucible + Lid + Hydrated compound 31.590g Hydrated Compound 1.004g
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NSS Chemistry Part 3 Metals HKCEE Past Paper Questions – Structural Questions 1. HKCEE 1995 Q1 Rubidium (Rb) and potassium belong to the same group in the Periodic Table. The relative atomic mass of rubidium is larger then that of potassium. (a) Explain whether rubidium is more reactive than potassium. (b) Write a chemical equation for the reaction between rubidium and water. (State symbols should be given.) (c) Suggest how rubidium can be stored safely in the laboratory.
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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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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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Beryllium and magnesium These are just like the reactions with dilute hydrochloric acid‚ and you have probably been familiar with the reaction between magnesium and dilute sulphuric acid almost since you started doing chemistry. Bubbles of hydrogen are formed‚ together with colourless solutions of beryllium or magnesium sulphate. For example: Calcium‚ strontium and barium Calcium sulphate is sparingly soluble‚ and you can think of strontium and barium sulphates as being insoluble
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Determination of Calcium ions in milk using titration. Background Calcium is a mineral which is essential to the human body. In fact 1.5% of the human body is made up of calcium‚ and not just the obvious uses such as bone and teeth formation but it is also a vital factor in many enzyme reactions‚ for example blood clotting. It also partakes in the regulation of the hearts rhythm. Lack of the crucial mineral can result in the build up of cadmium and lead‚ both of which are toxic. along
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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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