Reaction Procedure.1 l Begin the reaction. Add 10 ml of NaOH and the 80 ml of distilled water to a clean beaker and stir. 10 ml of NaOH 80 ml of dH 2 O10 ml of CV
Reaction Procedure.2 Add 10 ml of Crystal Violet solution to the beaker and stir.
Reaction Procedure.3 Obtain an aliquot of the reaction and place it in a cuvette. Insert the cuvette into the colorimeter and start recording the data with the CBL-2. Start
Reaction Procedure.4 l The calculator will display the data as it is collected and graphically track the progress of the reaction.
Reaction Procedure.5 l Once the CBL-2 has finished collecting data it will display a graph of the collected data.
Reaction Procedure.6 l Clean up all the glassware and the cuvette then return the equipment as directed. Rinse all glass ware with dH 2 O and dry before storing. Do not wipe the cuvette dry with any thing other than the optical wipes.
Data l In this experiment the data was automatically collected by the CBL-2 and stored in the graphing calculator. Nearly 200 data points were collected. For convenience they are not listed here.
Data Analysis.1 l The CBL-2 collected absorbance data. By using Beer’s Law we can conclude that absorbance is directly proportional to the concentration of the Crystal Violet indicator. Therefore absorbance data can be treated as concentration data.
Data Analysis.2 l In order to determine the order of the kinetics we need to evaluate how the concentration of Crystal Violet [CV] (absorbance data) changed with respect to time.
Data Analysis.3 l If the reaction is Zero Order then a graph of [CV] vs. Time will be linear. It’s not linear.
Data Analysis.5 l If the reaction is First Order then a graph of ln[CV] vs. Time will be linear. It’s Linear!
Data Analysis.6 l If the reaction is Second Order then a graph of 1 / [CV] vs. Time will be linear. It’s not.
Conclusion l Summarize the lab procedures. l Give the result(s). l Determine source(s) of error. l Describe an error propagation.