ChemLabSpring2007_Exp1_Solubility of Borax

ChemLabSpring2007_Exp1_Solubility of Borax - Experiment 1....

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Experiment 1. Thermodynamics: Determining the Enthalpy, Entropy, and Gibbs Free Energy of Solution for Borax by Measuring Ksp as a Function of Temperature 1. Purpose: The purpose of this experiment is to determine the effect temperature has on the solubility of Borax by calculating the number of moles needed to titrate 5mL of saturated Borax solution with .499M HCL at different temperatures. Then from that data calculating Ksp values at different temperatures and then using that to deterring the ΔG˚sol, ΔH˚sol, and ΔS˚sol. 2. Data: Personal Data Beaker Temperature (˚C) Level of HCl in Burette Start (mL) Level of HCl in Burette End (mL) Total HCl Added to the Beaker (mL) 1 20.8 0.19 5.50 5.31 2 21.0 5.61 10.30 4.69 3 21.8 10.30 15.17 4.87* 4 22.0 15.17 20.00 4.83* 5 22.0 20.00 24.72 4.72* *indicates a good trial John’s Section Data 3. Graphs and Table of Results All Section Data: Calculated Concentration of Tetraborate Ion, Ksp, and ΔGsol Actual Temperature in Celsius Moles of Sodium Tetraborate Present Concentration of Sodium Tetraborate (M) Ksp ΔG˚sol (J/mol) 10.3 0.000594 0.119 0.00670 11800 11.5 0.000699 0.140 0.0109 10700 21.9 0.00120 0.240 0.0553 7080 22.0 0.00125 0.251 0.0633 6750 29.8 0.00170 0.339 0.156 4660 Assigned Temp Actual Temp Volume HCl in Celsius in Celsius in mL 10 10.3 2.38 10 11.5 2.80 20 21.9 4.81 20 22.0 5.03 30 29.8 6.80 30 31.5 7.73 40 39.1 10.67 50 50.3 14.50 55 52.0 16.72 55 54.8 18.30
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ChemLabSpring2007_Exp1_Solubility of Borax - Experiment 1....

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