Equilibrium Constant lab report

Equilibrium Constant lab report - Taressa Cade Evaluation...

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Taressa Cade Evaluation the Equilibrium Constant Mr. Clark 3/31/08 Evaluating the Equilibrium Constant for the Reaction of Iron(III) Ion with Thiocyanate Ion Beginning question What is the significance of finding equilibrium constants of solutions? I predict that when solutions reach equilibrium, their molar concentrations can be used to determine the equilibrium constant. Safety Wear goggles Be aware of chemical hazards Avoid contact with skin Avoid inhaling the vapors and ingesting solutions Procedure 1. Label six 50 mL flasks S1 through S6. 2. Pipet 10 mL of 2.00x10-1M Fe(NO3)3 solution in each flasks. Pipet 1, 2, 3, 4, 5 mL of 2.00x10-3M NaSCN solution into flasks S2 through S6 respectively. Record concentrations of solutions from reagent bottles. Record the volume of NaSCN solution adding to flasks. 3. Add .10M nitric acid to each flask until the bottom of meniscus is even with the etched mark on the flask neck. Stopper the flask and invert each several times. 4. Set the wavelength of the spectrophotometer to 447 nm and adjust the %T reading to zero. 5. Obtain two cuvettet. Rinse one with solution S1; discard in a 600-mL beaker. Fill the rinsed cuvette with solution S1. Insert into the holder and adjust light control knob until the meter reads 100% T. 6. Rinse the second cuvette with solution S2 and discard. Fill the cuvette with S2 and insert into holder. Read and record %T. discard solution. 7. repeat step 6 using remaining solutions S3 through S6. Record %T for each. 8. Wash the cuvettes and flasks with soap and distilled water. Allow to dry. 9.
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This note was uploaded on 04/09/2008 for the course CHEM 1132 taught by Professor Cole/clark during the Spring '08 term at UCM.

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Equilibrium Constant lab report - Taressa Cade Evaluation...

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