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exp 5 - Experiment 5 Conductometric Titration Fall 2007...

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Experiment 5 – Conductometric Titration Fall 2007 Name Emily Winslett Lab Day and Time Tuesday, 1:00 TA Duy Le Section 409 Documentation Kenan Hill (Lab partner), Lab manual, pre-lab lecture Grading Rubric Possible Points Points Received Introduction 10 Purpose of report Goals of the experiment Materials and Methods 20 Describe procedure in paragraph format following guidelines provided (-2 for each type of mistake) Results and Discussion 50 Inserted titles for tables Inserted graphs into template Inserted captions for each graph Showed complete sample calculations Summarized all data in tables Answered questions completely Error analysis Laboratory Technique 20 TOTAL (100) TA Comments/Suggestions:
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C HEMISTRY 11L R EPORT T EMPLATE EXPT. Conductometric Titration 5 Introduction The purpose of this report is to determine the balanced chemical equation for calcium hydroxide (Ca(OH) 2 ) and phosphoric acid (H 3 PO 4 ) and compare the experimentally determined chemical equation with the theoretical balanced chemical equation. The objective of the experiment was to use a conductometric titration to measure the ion concentration in solution. Ion concentration in solution is directly related to the conductivity of the solution; therefore, as ion concentration decreases, so does the conductivity, and as the ion concentration increases, the conductivity increases as well. Materials and Methods A small weighing bottle without the lid was heated in the oven for 15 min. Once heated, this bottle was removed from the oven without tongs and then allowed to cool. Using a weighing boat and a scale approximately 1 g of calcium hydroxide (Ca(OH) 2 ) was measured and then placed into the weighing bottle. The bottle, again handled with tongs, was returned to the oven to dry for 2 hours. After two hours elapsed, the bottle was removed from the oven with tongs to cool for 10 min. The weighing bottle was then placed into a desiccator for a week until the next laboratory. The following week, the weighing bottle containing the calcium hydroxide sample was removed from the desiccator. The weighing bottle lid was placed on the bottle to keep the solid anhydrous. The weighing bottle was then placed on an electric scale to measure the mass, and the mass was recorded in Table 1. A scoopula was used to transfer ~0.05 g of calcium hydroxide from the weighing bottle into a 250-mL volumetric flask. The flask was placed on the electric balance, and calcium hydroxide was added to the flask until the mass was ~0.05 g. Once transferred, the mass of the weighing bottle was again measured to determine the mass of the calcium hydroxide transferred. The new mass of the weighing bottle was recorded in Table 1. The difference of the mass of the weighing bottle before the calcium hydroxide was removed and the mass of the weighing bottle after the calcium hydroxide was removed yielded the mass of the calcium hydroxide removed.
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