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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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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Materials: • Test tubes • Test tube rack • Test tube holder • 10 mL graduated cylinder • 100 ml beaker • Bunsen burner • Nichrome wire • Magnesium ribbon • Litmus paper(red) • Stirring rod • Crucible tong Procedures: We placed a pinch of NaCl‚ Na2CO3‚ and K2CO3 in
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of a Precipitation Reaction|Lab Section: | 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 __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
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a precipitation reaction. It is also to learn concepts of solubility and the formation of a precipitate. The Experiment and Observation: 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
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molecular form of the equation is Na2CO3.H2O + CaCl2.2H2O → CaCO3 + 2NaCl + 3H2O As the two reactant salts and sodium chloride are soluble in water but calcium carbonate is insoluble‚ the ionic equation for the reaction is that we present only the ions that react (after removing the spectator ions)we have the net equation as below CO32- (aq) + Ca2+(aq) CaCO3(s) From the balanced net ionic equation‚ 1 mole of carbonate ion from the 1 mole of Na2CO3.H2O(molar mass 124.00 g/mol)reacts
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the experiment: * Na2CO3(aq) + CaCl2. 2H2O(aq) à CaCO3(s) + 2NaCl(aq) + 2H2O * Put on your goggles. * Weigh out 1.0 g of CaCl2·2H2O and put it into the 100-mL beaker. Add 25 mL of distilled water and stir to form the calcium chloride solution. Use only distilled water since tap water may have impurities that interfere with the experiment.. Use stoichiometry to determine how much Na2CO3 you will need for a full reaction. * Weigh the calculated amount of Na2CO3 and put it in a small
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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 a perticipate
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Experiment 1: Calorimetry Nadya Patrica E. Sauza‚ Jelica D. Estacio Institute of Chemistry‚ University of the Philippines‚ Diliman‚ Quezon City 1101 Philippines Results and Discussion Eight Styrofoam ball calorimeters were calibrated. Five milliliters of 1M hydrochloric acid (HCl) was reacted with 10 ml of 1M sodium hydroxide (NaOH) in each calorimeter. The temperature before and after the reaction were recorded; the change in temperature (∆T) was calculated by subtracting the initial temperature
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It is so called since it can be easily removed simply by boiling with bicarbonates readily getting precipitated. Ca(HCO3)2 à CaCO3 + H2O + CO2 Mg(HCO3)2 à MgCO3 + H2O + CO2 Ca(HCO3)2 /Mg(HCO3)2 + 2C17H35COONa à (C17H35COO)2 Ca/Mg + 2 NaHCO3 CaCl2/MgCl2 + 2C17H35COONa à (C17H35COO)2Ca/Mg + 2NaCl CaSO4/MgSO4 + 2C17H35COONa à (C17H35COO)2 Ca/Mg + Na2SO4 2. Permanent Hardness/Non-alkaline/Non-carbonate is due to the presence of dissolved sulfates & chlorides of Ca‚ Mg‚ Fe‚ etc in water. Permanent
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