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Equilibrium and Le Chatelier’s Principle Lab

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on 6 March 2014

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Transcript of Equilibrium and Le Chatelier’s Principle Lab

Experiment 4
C0(H2O)6+2(aq) + 4Cl-(aq) CoCl4-2(aq) + 6H2O(l)
Experiment 1
NaCl(s) Na+(aq) + Cl-(aq)
Experiment 2
HIn(aq) H+(aq) + In-(aq)
Experiment 3
Fe+3(aq) + SCN-(aq) FeSCN+2(aq)
Conclusion
Experiment 4 (cont.)
effects of heat on the equilibrium of alcoholic cobalt (ethanol + cobalt(II) solution
Equilibrium and Le Chatelier’s Principle Lab
by Meredith Buckley
After mixing HCl with Saturated NaCl solution
Directly after adding Cl- ions (HCl-)
Saturated Salt Solution (NaCl + H2O)
Yellow
Blue
H2O and 0.1 M HCl mixed
Adding NaOH drop by drop to HCl solution
Trying to turn the solution green
Over-concentrated KSCN + Fe2(NO3)3 solution
Correct KSCN + Fe2(NO3)3 solution
Test tubes after equilibrium shifts
from right to left:
1) KSCN solution [control] 2) added crystals of KSCN 3) drops of Fe(NO3)3 solution 4) crystals of NaHPO4
H = +50 kJ/mol
Ethanol and Cobalt (II) Chloride solution
Test tubes with ethanol/cobalt (ii) chloride equilibrium shifts
from right to left:
1) alcoholic cobalt solution + drops H2O [control] 2) same as 1 + drops HCl 3) same as 1 + crystals NaCl 4) same as 1 + drops 0.1 M silver nitrate solution to form AgCl precipitate
Removing heat from the system
Adding heat to the system
-
H
Adding concentrations of OH- and H+ can greatly shift the equilibrium of any system. Sometimes, these shifts are apparent through physical changes. Colors, precipitates, and consistencies change due to shifts in the equilibrium.
HCl mixing into the solution is visible as HCl is thicker than water
Visible pieces of NaCl that formed upon adding HCl-
Original solution is yellow, portraying an acidic solution
Changes rapidly from yellow to blue
Perfect balance between HCl and NaOH to create green color
Added too much Fe(NO3)3 to water + KSCN solution
Made solution too dark to note any shift in equilibrium
Less concentrated; more H2O
Easier to note changes in equilibrium
"Purple" color
Creates alcoholic ethanol solution
Used only alcoholic ethanol solution + H2O; originally an almost clear, purplish solution
Immersed in boiling water, the solution slowly turned blue
Changed from blue slowly to an almost clear, pinkish solution closer to original state
Purpose
To observe shifts and changes in the equilibrium of various systems to learn and understand Le Chatelier's principle stating that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
Equilibrium isn't affected by the addition of a solid
Equilibrium shifts left to compensate for the added Cl- ions
Equilibrium is reached again with the precipitation of more NaCl to compensate for the added Cl- ions by shifting to the left
Equilibrium shifts to the left, reacting to the addition of H+ ions through the HCl+
Equilibrium shifts to the right, signaling a basic solution
Equal concentrations of strong acid (HCl+) and strong base (NaOH-) creating a pH 7 (neutral) solution
Control
Shifts Right
Shifts left
Neutralized
Control
Shifts Left
Shifts Right
Shifts Right
Shifts Left
Shifts to the left with the addition of heat
Removing heat shifts the equilibrium to the right
Endothermic reaction
Full transcript