The Earth’s atmosphere has changed over billions of years‚ but for the past 200 million years it has been much as it is today. We are‚ however‚ causing our atmosphere to change by human activity. Burning fossil fuels and deforestation are two examples of human effect on the environment. Composition of the Earth’s atmosphere The composition of air You need to know the proportions of the main gases in the atmosphere. The Earth’s atmosphere has remained much the same for the past 200 million years
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the gases‚ otherwise you can use the standard set up) The limestone cycle: 1. Burn the limestone chip/ limestone powder in a test tube in a Bunsen flame → calcium oxide 2. Put calcium oxide in water → calcium hydroxide solution + left over limestone 3. Filter the leftover limestone 4. Blow bubbles using a straw into the calcium hydroxide solution → limestone Flame colors: (I copied a table from the internet because it isn’t in the book‚ the ones in red I’m pretty sure you have to know‚ and the
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quantities. I have found that unknown sample B iron(iii) sulphate. I have identified it to be iron as it gave a yellow colour during the flame test narrowing it down to be barium or iron(iii). It then produced a yellow precipitate during sodium hydroxide test showing that it was iron(iii) instead of barium. The chemical equation for this reaction is: Fe2(SO4)3(aq) + NaOH(aq) Fe(OH)3(s) + Na2SO4(aq) I identified it as being a sulphate as it produced a white precipitate during the barium chloride
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Data Table: Qualitative Cation Tests Name Test Tube 1: HClNH3 Test Tube 2: NaOHExcess Aluminum 3+ No precipitate Slightly milky Dissolves Ammonium + No Precipitate No precipitate Calcium 2+ No Precipitate Milky white precipitate Precipitate does not dissolve Copper 2+ No precipitate Became much darker blue and milky Iron 3+ Brighter yellow Orange precipitate that then dissolves Lead 2+ Milky white precipitate Precipitate gets more milky Silver + Milky white precipitate Precipitate gets
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analysis of ions present in a solution. A large industry that employs this type of chemistry is the mining industry. In the mining industry metals are not typically pure when first collected. Through the use of selective precipitation and the knowledge of Ksp values‚ certain metal ions can be precipitated out. EXPERIMENTAL The Selective Precipitation of the Barium Magnesium Group experiment instructions were followed directly from the handout printed from the course website. RESULTS AND REVIEW
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a pH of 2-3. When too much of this acid is formed in the stomach‚ heartburn and other discomfort occurs. This is when people grab for their antacids; these are bases that neutralize the excess acid in the stomach. Calcium carbonate‚ magnesium hydroxide‚ and aluminum hydroxide are all examples of bases used in antacids. In addition to these active ingredients‚ antacids also contain sweeteners‚ colourings‚ and “fillers” that may or may not affect the effectiveness of the neutralization. This
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(b) Calcium oxide CaO (c) Aluminum nitride AlN (d) Beryllium chloride BeCl2 (e) Potassium iodide KI (f) Aluminum oxide Al2O3 23. Write the correct formula for the following binary molecular compounds. (a) Carbon monoxide CO (b) Boron tribromide BBr3 (c) Sulfur hexafluoride SF6 (d) Carbon dioxide CO2 (e) Carbon tetrabromide CBr4 (f) Nitrogen dioxide NO2 24. Write the correct formulas for the following compounds that contain polyatomic ions. (a) Sodium hydroxide NaOH
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neutralize stomach acid. They are used to relieve acid indigestion‚ upset stomach‚ sour stomach‚ and heartburn. Antacids are taken by mouth and work by neutralizing excess stomach acid. They contain ingredients such as aluminum hydroxide‚ calcium carbonate‚ magnesium hydroxide‚ and sodium bicarbonate‚ alone or in various combinations. Antacid products may also contain other ingredients such as simethicone‚ which relieves gas. Antacids differ in how quickly they work and how long they
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70 14 73 15 40 16 79 17 80 18 84 12 45 48 51 52 55 56 59 59 64 65 75 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton 24 96 25 31 115 32 119 33 122 34 128 35 127
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of Different Cations When they were heated by Fire. & Testing changes of cations using sodium hydroxide (NaOH) aqueous Aims & Objectives Different characteristic cations will form different colors when they are burned or added base. In these two experiments‚ scientist took some sample of barium hydroxide (Ba (OH) 2·H2O)‚ ferric chloride (FeCl3·6H2O)‚ copper chloride (CuCl2· 2H2O)‚ calcium chloride anhydrous (CaCl2)‚ potassium carbonate crystal (K2CO3· 2H2O)‚ strontium chloride hexahydrate
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