precipitate reaction that yielded 2.00 grams of CaCo3‚ then we looked at the ratio of moles reactant to moles product. We then substituted the ratio of the molar mass of each reactant to molar mass of the product in for each mole. We divided this to find out how many grams of reactant for every one gram of product‚ and finally multiplied this by two. Our final results were lower than the desired 2.00 grams. Balanced Equation: CaCl2 X 2H2O + Na2CO3 x H2O → CaCO3 + 2NaCl + 3H2O Background Information:
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are a. Provide protection to the distribution system to prevent corrosion b. Add minerals that are 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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Answer Paper for Science and Technology - II - Paper 4 Time: 2.0 Hrs.------------------------------------------------------------------------------------Max. Marks: 40 Note 1). All questions are compulsory. Note 2). All questions carry equal marks. Note 3). Draw neat and labelled diagrams wherever necessary. Important note from mySSC.in - In this ’Answer paper’‚ questions are displayed for your convenience. In actual exam‚ do not write the questions. Only answers are expected in answer paper
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AP Chemistry Chapter 17 Additional Aspects of Aqueous Equilibria Chapter 17. Additional Aspects of Equilibrium Common Student Misconceptions • • • • • Students often believe that the pH at the equivalence point for any titration is 7.00. In terms of problem-solving skills‚ this is probably the most difficult chapter for most students. Students tend to find buffers particularly difficult to understand. Students often forget to consider volume changes that occur when two solutions
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KWAME NKRUMAH UNIVERSITY OF SCIENCE AND TECHNOLOGY COLLEGE OF TITLE: REMOVAL OF HARDNESS OF WATER USING PRECIPITATION AND COMPLEXATION METHODS. NAME: KWARTENG YAW PRINCE COURSE: BSC. ENVIRONMENTAL SCIENCE YEAR: FIRST YEAR EXPERIMENT NO. : A.1.1.3. T.A.: BRIGHT KOFI LEONARD DATE: 7TH NOVEMBER‚ 2007. Aims and Objectives: 1. To describe water hardness.
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will test for the formation of copper (ii) oxide and carbon dioxide. Limewater is a sensitive test for CO2‚ forming a distinctive milky precipitate: CO2(g) + Ca(OH)2(aq) arrow CaCO3(s) + H2O(l) Calcium carbonate is strongly heated until it undergoes thermal decomposition to form calcium oxide and carbon dioxide CaCO3 CaO + CO2 Other metal carbonates decompose in the same way. Here are the equations for the thermal decomposition of copper carbonate: copper carbonate copper oxide + carbon dioxide
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Scheme of Analysis for Unknown 9A/9B “Fair Game” Unknowns * Cations: Na+‚ K+‚ NH4+‚ Ca2+‚ Mg(H2O)62+‚ Al(H2O)63+‚ Zn(H2O)62+‚ Cu(H2O)2+‚ Ag(H2O)+ * Anions: Cl-‚ NO3-‚ SO4-2‚ HSO4-‚ OH-‚ CO3-2‚ HCO3-‚ S-2 * Insoluble Salts: Ca(OH)2‚ CaCO3‚ CaSO4‚ Mg(OH)2‚ MgCO3‚ Ag2O‚ AgCl‚ Ag2S‚ CuO‚ CuCO3‚ CuS‚ Zn(OH)2‚ ZnCO3‚ ZnS * Alums: [Al(OH2)6]2(SO4)3∙6H2O‚ Na[Al(OH2)6](SO4)2∙6H2O‚ K[Al(OH2)6](SO4)2∙6H2O‚ NH4[Al(OH2)6]2(SO4)2∙6H2O * Hydrated Ions: Na2CO3∙10H2O‚ Na2SO4∙10H2O‚ Ca(OH2)6Cl2
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chemical reaction. Once the titration is complete you can calculate your water hardness. The formula used to calculate the water hardness is as followed: Mg Caco3/1L CaCO3 soln= VmL Na2EDTA soln/0.02500L CaCO3 soln x M mol Na2EDTA/1L Na2EDTA soln x 1 mol CaCO3/1 mol Na2EDTA x 100.1g CaCO3/ 1 mol CaCO3/1 mol Na2EDTA x 100.1 g CaC03/ 1 mol CaCO3 Above in the formula V represents the actual delivered volume of Na2EDTA solution and M is your actual molarity. Procedures: Start by preparing 500mL of
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Assignment 1. Questions from chapters 1 and 2 of McMurry and Fay Question numbers are from the fourth edition. Chapter 1. Chemistry: Matter and Measurement 1 1.1 1.2 1.3 (a) Cd (b) Sb (a) silver (c) Am (c) rhenium (d) cesium (e) argon (f) arsenic (b) rhodium (a) Ti‚ metal (d) Sc‚ metal (b) Te‚ semimetal (e) At‚ semimetal (c) Se‚ nonmetal (f) Ar‚ nonmetal 1.4 1.5 The three Acoinage metals@ are copper (Cu)‚ silver (Ag)‚ and gold (Au). (a) The decimal point must be shifted
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1. Identify the natural sources of sulphur dioxide and oxides of nitrogen. SO2‚ natural: - Geothermal hot springs and volcanic activity are natural sources of SO2. - In the process of decaying of organic matter some bacteria will produces hydrogen sulphide as a waste product which will oxidise‚ forming so2. - Phytoplankton release dimethyl sulphide (DMS) into the atmosphere‚ when this is oxidised it forms sulphuric acid. NOx‚ natural: - Lightning activity generates high temperatures to allow
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