TABLE OF CONTENTS 1. IA (Alkaline Metals) 1.1. H………………………………………………………………………..2 1.2. Li………………………………………………………………………..2 1.3. Na………………………………………………………………………2 1.4. K………………………………………………………………………..3 1.5. Rb………………………………………………………………………3 1.6. Cs………………………………………………………………………3 1.7. Fr……………………………………………………………………….4 1. IIA (Alkaline Earth Metals) 2.8. Be………………………………………………………………………4 2.9. Mg………………………………………………………………………4 2.10. Ca………………………………………………………………………4
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what you add and what happens when you add it. Remember‚ you cannot add single ions‚ only compounds or aqueous solutions of the compounds. a. Ba2+‚ Mg2+ and Na+ b. Ag+‚ Cu2+ and Mg2+ 16. Complete the balanced dissociation equation and write the Ksp equation for the following dissolving substances. a. CaCO3(s)
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with the calcium in lime scale. It is safe to use because it does not produce chlorine gas [5]‚ which can be toxic. Sulfamic acid also has a low volatility. Disadvantages: Sulfamic Acid can be an irritant to eyes or skin and is the most expensive of the de-scalers. Q2) How these de-scalers remove limescale Limescale forms when hard water is heated above 61°C or when it is left to evaporate on surfaces such as taps and showerheads. Hard water is water that contains high quantities of calcium and magnesium
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PROCEDURE: Pre Lab: The experiment should be carried out AWAY from the sunlight. Before beginning the experiment‚ we need to make sure that the benzene used in the experiment is free of toluene and water. To do this‚ we must put anhydrous calcium chloride into a flask of benzene to "dry" it and remove the toluene. This is then decanted into a vacuum filter‚ which will leave only pure benzene. Synthesis of Bromobenzene: Set up a reflux and place in a cold-water bath. In addition to setting
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Different types of fireworks would have different elements or compounds in them. b.) If you wanted red fireworks‚ you could use lithium nitrate or lithium chloride. For orange‚ use potassium nitrate‚ calcium nitrate or sodium nitrate. For yellow fireworks use barium nitrate. If you wanted green fireworks use copper II nitrate or copper II chloride. Limitations to compounds you can use in fireworks is you need to make sure they are not toxic‚ so certain colours may not be
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the non-metal that is responsible for the colour produced in the flame test for that salt. How can you be sure your answer is correct? Metal is responsible for the colour produced in the flame test for that salt. All salts contain chloride ion. If non-metal ion‚ chloride‚ is responsible for the colour‚ all colour produced will be the same. 3. Why do the chemicals have to be heated in the flame before the coloured light is emitted? For the coloured light to be emitted‚ the electrons have to get
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Contents 1) Sulphuric Acid----------------------------------------------------------------(1-6) a. Uses of sulphuric b. Manufacture of sulphuric acid c. Sulphur dioxide and environmental pollution 2) Ammonia and Its Salt-----------------------------------------------------(7-10) d. Uses of ammonia e. The properties of ammonia f. Manufacture of ammonia g. Preparation of ammonium fertilisers 3) Alloys------------------------------------------------------------------------(11-14)
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In this lab we tested the purity of water by looking for the chemicals free chlorine‚ chloride‚ sulfate‚ nitrate‚ copper‚ total hardness‚ iron‚ hydrogen sulfide‚ lead‚ pesticides‚ pH‚ total alkalinity‚ and total chlorine inside a water sample. The chemicals that produced a 0.0 result meant that there was no trace of that chemical inside the sample. The chemicals not found were copper‚ hydrogen sulfide‚ free chlorine‚ lead‚ iron‚ pesticide‚ and total chlorine. As a class we found the results of
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and Na2CO3 __0.72__g Net mass of the Na2CO3 ___0.12_g Step 6: Mass of filter paper __1.0__g Step 10: Mass of filter paper and dry calcium carbonate __1.7__g Net mass of the dry calcium carbonate ___0.7_g (This is the actual yield) Step 11: Show the calculation of the theoretical yield of calcium carbonate. .0068 mol of CaCO3 *100.06 g CaCO3/1mol of CaCO3 =.6804 g of CaCO3 Show the calculation of the percent yield. (Actual yield/theoretical yield)*100
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Weigh out your 1.0g of CaCl2-2H20 and put it into the 100mL beaker‚ Add your 25mL of distilled water and stir to form the calcium chloride solution. Next‚ use stoichiometry to determine how much Na2CO3 and put it into a small paper cup. Then add the 25mL of distilled water to make the sodium carbonate solution. Mix the two solutions in the beaker and a precipitate of calcium carbonate will form instantly. Next set up your filtration assembly. After the filtration assembly is ready‚ swirl the contents
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