AP Chemistry Analysis of Alum * Purpose: * In this lab we performed several tests to determine if our crystals were actually aluminum potassium sulfate. * Procedures: * Materials: * Chemicals: * Aluminum potassium sulfate‚ 2.5 g * Equipment – Part 1: * 150 mL beaker * Bunsen burner * 2 capillary tubes * Mortar and pestle * Notched stopper to hold thermometer *
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the formation of a precipitate. Materiel needed: Test tubes Rack of test tubes Plastic droppers Beakers Procedure: We prepare 7 beakers of 7 different solutions (that we mark from 1→ 7). We put separately around 50 ml of: HCl NaOH Na2CO3 K2CrO4 CaCl2 CuSO4 Unknown substance Using plastic droppers we mix 10 drops of one solution with 10 drops of another solution in a test tube‚ to get all in all 20 different test tubes. We then note the observation for each test tube. Name
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Aim: To compare the foaming capacities of five different commercial soaps. Apparatus: 5 test tubes‚ 5 conical flasks (100 ml)‚ test tube stand‚ Bunsen burner and stop watch. Materials Required: 5 different samples of soap and distilled water Theory: The foaming capacity of a soap sample depends upon the nature of soap and its concentration. This can be compared for various samples of soaps by taking the same concentration of solution and shaking them.The foam is formed and the time taken
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Precipitation Reaction|Lab Section: 73426| Data Tables: Step 3: Show the calculation of the needed amount of Na2CO3 CaCl2.H2O(aq)= m/M =1/147 =0.0068 mol CaCO3(s)=0.0068*1/1 =0.0068 mol CaCO3(s)= CaCO3 (s)= CaCO3 mol *CaCO3 g =0.0068 mol*100.01 g =.68 g Step 4: Mass of weighing dish _0.6_g Mass of weighing dish and Na2CO3 .72_g Net mass of the Na2CO3 .12_g Step 6: Mass of filter paper __1.0__g Step 10: Mass of filter paper and dry calcium
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we determined the activity order of the metals used based upon our results. Data Sheet: Part A: Reaction #1A: Na2CO3(aq) + HCL(aq)(0.5m) H2CO3(g) + 2NaCl(l) H2O(l) + CO2(g) + 2NaCl(l) Observations: There was a formation of a gas and the liquid was clear. Reaction #2A: Na2CO3(aq) + NaCl(aq) Na2CO3(aq) + NaCl(aq) Observation: No reaction was observed. Reaction#3A: Na2CO3(aq) + CaCl2(aq) 2NaCl(aq) + CaCO3(s) Observations: The solution turned white and cloudy which is evidence that
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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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Aim: To determine the water of crystallization in washing soda crystals (Na2CO3.xH2O) Research Question: What is the percentage composition and the amount (in moles) of water in the given ionic hydrate? (Na2CO3.xH2O) Background Information: Sodium Carbonate also known as Washing Soda (Na2CO3.xH2O) is a sodium salt of carbonic acid. Sodium carbonate is domestically well known for its everyday use as a water softener. It is also used to remove grease‚ oil and wine stains. It can be extracted from
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| | KCl | Na2SO4 | NaOH | Na2CO3 | Test solutions | SrCl2 | No reaction | Reaction | Reaction | Reaction | | AgNO3 | Reaction | Reaction | Reaction | Reaction | | BaCl2 | No reaction | Reaction | Reaction | Reaction | | MgCl2 | No reaction | No reaction | Reaction | Reaction | Data Balanced equations: SrCl2 (aq) + KCl (aq) NO REACTION SrCl2 (aq) + Na2SO4 (aq) SrSO4 (s) + 2NaCl (aq) SrCl2 (aq) + 2NaOH (aq) Sr(OH)2 (s)+ 2NaCl (aq) SrCl2 (aq) + Na2CO3 (aq) SrCO3 (s) + 2NaCl (aq)
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weight of the calcium carbonate. This is your actual yield of calcium carbonate. 11. Now calculate the percent yield‚ using your theoretical yield and actual yield. Make sure to show all stoichiometric calculations and all data in your lab report. Na2CO3(aq) + CaCl2. 2H2O(aq) → CaCO3(s) + 2NaCl(aq) + 2H2O Data‚ observations‚
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Ca(s) +H2O->Ca (OH)2(aq)+H2(g) Step 4: Mg(s) +H2O->Mg (OH)2(aq)+H2(g) Step 10: CaSO4 + H2O-> Ca(OH)2 + H2SO4 MgSO4 + H2O ->Mg (OH)2 + H2SO4 Barium Sulfate: No reaction Step 13: MgCl2 + Na2CO3 -> MgCO3 + 2NaCl CaCl2 + Na2CO3 -> CaCO3 + 2NaCl BaCl2 + Na2CO3 -> BaCO3 + 2NaCl 2. The reactivity of the metal increases with each period it goes down. Magnesium is the least reactive and is in the third period with an atomic number of 12. Calcium is slightly more reactive
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