Experiment 3: Stoichiometry of a Precipitation Reaction Abstract: In this experiment the objectives were to try and predict the amount of product that was produced in the precipitation reaction of calcium carbonate by using stoichiometry. Then learn how to figure out the actual yield‚ theoretical yield and percent yield of the experiment. Experiment and Observation: The first step in the experiment was to weigh 1g of CaCl2 +2 H2O‚ then pour it into the 100mL
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calcium ion solution had to be converted to M so 1g/L/100.1g=.009990M calcium ion solution. Titration 1: 10.00mL CaCO3; .00999MCaCO3X.0100L= .0000999mol CaCO3 .0000999mol EDTA/.002507L = .00398M Na2EDTA Titration 2: 10.00mL CaCO3; .00999MCaCO3X.0100L= .0000999mol CaCO3 .0000999mol EDTA/.02339L = .004271M Na2EDTA Titration 3: 9.95mL CaCO3; .00999MCaCO3X.0100L= .0000994mol CaCO3 .0000994mol EDTA/.02367L = .004196M Na2EDTA Since the first titration is so far out from the other two it was thrown
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name‚ date‚ and CaCO3 . 16. When the filtration process is complete‚ place the filter paper and the solid CaCO3 product on the labeled watch-glass. 17. Leave your labeled watch glass out for drying overnight (low temperature). 18. Record the mass of the dry filter paper + CaCO3. Record mass Questions and answers for Limiting Reactant 1. The mole of Na2CO3 used is n= m÷M = 3.01g÷105.99 =0.028mol 2. The moles of CaCO3 n= m÷M = 4g÷100.09g/mol =0.040 mol 3a: mass of CaCO3 produced is
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we have a balanced 1:1 ratio and have 0.0068 mol of CaCl2 then we will get 0.0068 mol of CaCO3 which turns out to be 0.68g of CaCO3. 0.0068 mol CaCO3*100.09g/mol CaCO3 = 0.68 g CaCO3 B. According to your data table‚ what is the actual yield of the product? 0.6 grams CaCO3 (However the scale actually tipped 1.7g and 1.6g and finally settled on 1.6g) C. What is the percent yield? 0.6g CaCO3/0.68g CaCO3 = 0.88*100% = 88% yield D. A perfect percent yield would be 100%. Based on your results
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Unit Plan On Acids & Bases May 25‚ 2006 Table of Contents I. General Objectives Page 3 II. Learning Outcomes Page 4 III. Assessment‚ Grading & Resources Page 5 IV. Tending to different Learning styles Page 7 V. Schedule Page 8 VI. Appendix 1 Page 20 Acids and bases Unit plan Grade 12 General Objectives: ▪ Introduce pH‚ acid and base definition ▪ Discuss acid
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Determining the Limiting Reactant and Percent Yield in a Precipitation Reaction Objectives: Observe the reaction between solutions of sodium carbonate and calcium chloride. Determine which of the reactants is the limiting reactant and which is the excess reactant. Determine the theoretical mass of precipitate that should form. Compare the actual mass with the theoretical mass of precipitate and calculate the percent yield. Materials: Balance 0.70 M sodium carbonate solution‚ Na2CO3(aq)
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Separation Techniques Aim: To separate a mixture of Iron filings‚ CaCO3‚ NaCl into their pure substances. Apparatus: • 2x 150ml beakers • 1x 150Ml Beaker • Magnet • Matches • Evaporating basin • Bunsen Burner • Water • Funnel • Retort stand • Funnel Paper • Sieve • Iron Filings • CaCO3 • NaCl • tripod • Gauze Mat • Cling Wrap • Saftey Goggles Method: 1. Gather Apparatus and the mixture of Iron‚ CaCO3 and NaCl. 2. Weigh beaker and mixture. 3. Use magnetic separation
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Aim: To investigate the rate of thermal decomposition of CaCO3 at different temperatures. Research Question How does temperature influence the rate of thermal decomposition in CaCO3? Hypothesis Every time more heat is added to the element‚ CaCO3‚ thermal decomposition will take place faster because the heat is a catalyst which speeds up the reaction. Variables Dependent Variables → Mass of Calcium Carbonate Independent Variables → Temperature Controlled Variables → Calcium Carbonate
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The unknown carbonate was classified as K2CO3. This was supported by the data collected. For example‚ the measured mass of 1.3 for the precipitated CaCO3 found in Data Table 1: Mass of Important Objects was used to determined the molar mass of M2CO3‚ which was 146.15 g/mol. Based off the possible unknowns‚ K2CO3 had the closest molar mass which was 138.21. This supports the claim that the unknown
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Title: Determination of Water Hardness Using a Titrator Purpose: To become familiar with the concept of water hardness‚ practice a titration technique using a titrator‚ and determine the hardness of the local water supply. Procedure: 1. Gather the test tube holder‚ small stopcock‚ 10-mL syringe (titrator)‚ and 2 thick textbooks and the LabPaq box or 5-6 thick textbooks. 2. Remove the plunger from the titrator and place it back in your LabPaq box. 3. Attach the stopcock to the tip of
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