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CHM110 Experiment 2 Final Report.docx

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University of Toronto Mississauga
Judith C Poe

EXPERIMENT - 2 DETERMINE THE PRODUCT OF A REDOX REACTION REACTION OF BROMATE AND HYDROXYLAMMONIUM IONS CHM110H5F EXPERIMENT PERFORME03 OCTOBER, 2012 REPORT SUBMITTED10 OCTOBER, 2012 SUBMITTED MATTHEW DACOSTA P a g e | 1 I. Purpose: The purpose of the experiment was to find the equation of the redox reaction with the help of quantitative and qualitative analysis of the reaction where Bromate ions and Hydroxylammonium ions are reacted to find the identity of the nitrogen containing product. 2 II. Experimental method 1. Using a burette, 20mL solution of KBrO was 3easured and transferred into a 250mL Erlenmeyer flask. 2. A 10mL of NH OHCL3solution was measured using a volumetric pipette and delivered it into the Erlenmeyer flask. 3. Then, with a graduated cylinder, 15mL of Hydrochloric acid was introduced into the mixture and the flask was kept under a fume hood to ensure any gas that evolved during the reaction escaped through the fume hood. 4. The mixture was mixed thoroughly by swirling and the flask and was allowed to rest under the fume hood with a watch glass covering the opening of the flask. 5. During the resting period, close observations were made with regards to color and temperature changes, any evidence of gas formation etc. 6. While the mixture was resting under the fume hood, a burette was taken and rinsed with sodium thiosulfate solution. Then, it was filled with the stock solution and the initial reading of the burette was noted. 7. After 10 minutes of reaction period, the flask was removed from the fume hood and 5mL of potassium iodate solution was added to the mixture and mixed well. 8. The mixture was immediately titrated with the sodium thiosulfate solution from the burette until the solution in the Erlenmeyer flask turned pale yellow. 9. A 2mL of starch solution was added to the flask. Since the titration was done accurately, the solution changed into a deep blue color P a g e | 2 10. Following the color change, drop wise titration was performed to ensure that the equivalence point was reached as accurately as possible. 11. The final reading of the burette was noted down and the volume of Na S O used to titrate was 2 2 3 calculated by calculating the difference between the initial and the final burette readings. 12. The procedure was repeated 3 times and the results were averaged to arrive at the best possible answer. III. Collection of Data Refer to Data Sheet in the Appendix IV. Results and Calculations From conducting the experiment, the following data was obtained. Trial # Volume of KBrO (0.3200M) Volume of Na S2O 2031003M) Trial 1 20.00mL 12.00mL Trial 2 20.00mL 10.60mL Trial 3 20.00mL 10.75mL Table 1.1 – Volume of KBrO t3trated with Na2 2O 3for more details, refer to appendix) Number of moles of Na S O and KBrO was calculated using where ‘n’ is the number of moles 2 2 3 3 and ‘M’ is the Molarity of the given solution and ‘v’ is the volume of the given solution . BrO + 9I + 6H O → Br + 3 I + 9H O---------- Equation ① 3 3 3 2 - - - - [I3+ 2S 2 →33I + S O ] 4 6 -------------------- Equation ② BrO + 6S O + 6H O → Br + 9H O + 3S O ---------- Equation ③ ( Equation ① + ②) 3 2 3 3 2 4 6 By adding Equation ① and Equation ② , the following observations were made. P a g e | 3 -
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