Equilibrium Lab

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CJ Tavner
2/04/2013
Chemistry Lab: Equilibrium and LeChatelier’s Princinple

Objective: Put stresses on the systems; observe how the equilibrium’s systems react to a stress. Materials and Procedures:
A. Materials
1. NaCl(s)
2. KSCN, 0.002M
3. Bromythymol blue indicator solution
4. AgNO3, 0.1
5. CoCL2 x 6H2O(s)
6. HCl, 12M
7. HCL, 0.1M
8. NaOH, 0.1M
9. Fe(NO3)3, 0.2M
10. C2H5OH(l)
11. Na2HPO4(s)
12. Test tubes
13. Beaker
14. Stirring rod
15. Test tube rack
16. Graduated cylinders
17. Funnel, filter paper, and holder for funnel
B. Procedure:
1. Equilibrium in a Saturated Solution
You will investigate the equilibrium in saturated sodium chloride solution: NaCl(s) (( Na+(aq) + Cl-(aq)
Pour some solid NaCL into a test tube and fill the tube about ¾ full of distilled water. Cork and shake to form a saturated solution. If all the NaCl dissolves, pour some additional NaCl in the tube and shake until a saturated solution with some excess solid is obtained. Filter the solution into a second test tube. To this saturated solution of NaCl, add some Cl- ions in the form of concentrated HCl. Record and explain the results. 2. An Acid-Base Indicator Equilibrium

Acid-base indicators are large organic molecules that can gain and lose hydrogen ions to form substances that have different colors. The reaction of the indicator bromthymol blue can be illustrated as follows: HIn(aq) (( H+(aq) + In-(aq) In this reaction HIn is the neutral indicator molecule, and In- is the indicator ion after the molecule has lost a hydrogen ion. Equilibrium reactions can easily be forced to go in either direction. Reactions like this are said to be reversible. Fill a small test tube about half-full of distilled water. Add several drops of bromthymol blue indicator solution. Add 5 drops of 0.1M...
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