Lab Report for Experiment #10 Stoichiometry of a Precipitation Reaction Student’s Name ____________________ Date of Experiment ___________ Date Report Submitted _________________ Title: Purpose: Instructor Changes: Weigh out about 1.7 g of CaCl2·2H2O and record your mass to +/- 0.1 g (for example 1.6 g‚ 1.7 g‚ or 1.8 g). We have made this change so that you will have 2 sig figs in subsequent calculations. Have you made any changes to the procedure? Please explain: Data Tables and Observation:
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conducted by dissolving three ionic compounds‚ CaCl2‚ Na2CO3‚ and NaCl‚ in distilled water to measure the enthalpy of solution.
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of CaCl2·2H2O‚ stoichiometric calculations should give the following results: 1 g CaCl2·2H2O x 1 mole CaCl2·2H2O x 1 mol Na2C03 x 106 g Na2C03 = 147 g CaCl2·2H2O 1 mol CaCl2·2H2O 1 mol Na2C03 Using 1 g of CaCl2·2H2O and .72 or .8 g (slight excess) Na2CO3 Should give a CaCO3 theoretical yield as follows: 1 g CaCl2·2H2O x 1 mole CaCl2·2H2O x 1 mol CaC03 x 100 g CaC03 = 147 g CaCl2·2H2O 1 mol CaCl2·2H2O 1 mol CaC03 To double-check‚ we can calculate CaCO3 theoretical yield by using Na2CO3 0.72
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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 of the unknown
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part of chemistry. In this experiment‚ you will react a known amount of sodium carbonate solution with a known amount of calcium chloride solution. The skeletal (unbalanced) equation for the resulting double replacement reaction is: Na2CO3(aq) + CaCl2(aq) Æ NaCl(aq) + CaCO3(s) Note that three of the chemicals have their states or phases designated as (aq) and one is designated as (s). The (aq) represents the term aqueous which means that the substance is soluble and dissolved in water
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Paper towels 1 Small paper cup 1 Coffee cup or mug 1 Beaker‚ 100 mL‚ glass 1 Funnel 1 Cylinder‚ 25 mL 1 Goggles-Safety 1 Scale-Digital-500g 1 Weighing boat‚ Plastic 1 CaCl2·2 H2O-Calcium Chloride‚ Dihydrate - 2.5 g 1 Filter Paper 12.5-cm 1 NaCO3-Sodium Carbonate - 2 g Procedure 1. Put on your goggles. 2. 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
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OBSERVATIONS (15 points) INSERT THE FOLLOWING DIGITAL PHOTOGRAPHS OF YOURSELF : (5 points) * Measuring the CaCl2 * Stirring the reaction mixture * Folding the filter paper * Pouring the reaction mixture into the filter paper in the funnel * Placing the product on the paper towels to dry Experimental Step | Observations | Mass of CaCl2•2 H2O used (grams) | | Mass of Na2CO3 used (grams) | | Net mass of mixture‚ grams | | Appearance of mixture when the reactants are mixed
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Purpose: The purpose is to predict the amount of precipitation using stoichiometry. Another purpose is to measure and calculate percentage yield. Procedure: 1. Weigh out 1.0g of CaCl2*2H2O and put it into a 100mL beaker. 2. Add 25mL of distilled water and stir. 3. Using stoichiometry to determine how much Na2CO3 is needed for a full reaction. 4. Weigh the calculated amount and put it in a small paper cup. Add 25mL distilled water and stir. 5. Pour this solution into the beaker and watch
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sodium carbonate solution‚ Na2CO3(aq) Graduated cylinder 0.50 M calcium chloride solution‚ CaCl2(aq) Beaker (250 mL) Wash Bottle (distilled H2O) Filter paper Funnel Iron ring Ring stand Procedure: Part I: The Precipitation Reaction (Day 1) 1. Obtain two clean‚ dry 25 mL graduated cylinders and one 250 mL beaker. 2. In one of the graduated cylinders‚ measure 25 mL of the Na2CO3 solution. In the other graduated cylinder‚ measure 25 mL of the CaCl2 solution. Record these volumes
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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 mol *CaCO3 g =0.0068 mol*100.01 g =0.68 g Convert moles of Na-2CO3 to grams of Na2CO3 = 0.00680 moles Na-2CO3 x 105.99g Na-2CO3 1 mole Na-2CO3 = 0.72g 0.72g of Na-2CO3 to fully react with 1g of CaCl2-.2H2O Step 4: Mass of weighing dish _0.5_g Mass of weighing dish and Na2CO3 _1.2_g Net mass of the Na2CO3 _0.7__g Step 6:
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