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8/12/2019 Ppt Chemical Equilibrium
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8/12/2019 Ppt Chemical Equilibrium
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Chemical equilibrium is the condition which occurs when the
concentration of reactants and products participating in a
chemical reaction exhibit no net change over time. Chemical
equilibrium may also be called a "steady state reaction."
Le Chatelier principle said that : If a system at equilibrium is
subjected to a change of pressure, temperature, or the number
of moles of a component, there will be a tendency for a net
reaction in the direction that reduces the effect of this change.
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1. What is the factor that effecting chemical equilibrium?
2. What is the effect of adding concentration of chemicalsubstance to the chemical equilibrium?
3.Does the additional of different substance make the
same effect to the solution?
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To prove Le Chateliers Principle
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If we adding substance to the
equilibrium system, then the composition
of the system will tend to change untilthat new equilibrium state is attained.
The changing can be in form of color
changing.
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3. Can predict the changing that appear from
chemical equilibrium reaction.
1. The observer can understand about Le Chatelier
2.Do the experiment of chemical equilibrium properly.
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What is the Le Chtelier PrincipleLe Chtelier principle: If a system at equilibrium
is subjected to a change of pressure, temperature, or
the number of moles of a component, there will be a
tendency for a net reaction in the direction that
reduces the effect of this change.
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No Materials Amount
1 KSCN 0,01 M 2 mL
2 FeCl30,01 M2 mL
3 H2C2O4 0,01 M 2 mL
4 K2Cr2O70,01 M1 mL
5 HCl 0,01 M As much as drop of NaOH 0,01 M
6 NaOH 0,01 MCount the drop that change the
color
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2 mL of KSCN 0.01 M was taken
All of the equipment were cleanedand dried.
All of the materials and equipments wereprepared.
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HCl 0.1 M was added into test tube 2 as much asNaOH 0.1 M
1 mL of K2Cr2O70.01 M was obtained of each into 2 test tube.
Test tube 1 was used as standard.NaOH 0.1 M was added into test tube 2 until the colour
change. (The drops that changed the colour was counted)
2 mL of FeCl3 was added into the test tube containing KSCN. The
appearance was noted. The liquid was divided into four test tube.The test tube 1 was used as standard
2 mL of KSCN wasadded into test tube 2
2 mL of FeCl3was addedinto test tube 3
2 mL of H2C2O4 wasadded into test tube 4.
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1 2 mL KSCN + 2 mL
FeCl3
(Standard )
Red
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2 Standard +
2 mL KSCN
SCN- RED Right to the left
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3 Standard +
2 mL FeCl3
Fe3+ Red darker Right to the left
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4 Standard +
2 mL H2C2O4
C2O42
-
Yellow Left to the right
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No Solution Drop
NaOH
Color Equilibrium
1 K2Cr2O70,01 M 25 Yellow To the left
2 K2Cr2O70,01 M 11 Yellow To the left
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No Solution Drop HCl Color Equilibrium
1 K2Cr2O70,01 M 25 Orange To the right
2 K2Cr2O70,01 M 11 Orange To the right
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When KSCN added by FeCl3 itllbe formed Iron(III) Tiocyanate
[Fe(SCN)3] which easy to soluble in water and produce red color
sulution. The red color of solution is caused by ion hydrazed by
FeSCN2+.
The reaction is :
3 KSCN (aq) + FeCl3 (aq)Fe(SCN)3(aq) + 3 KCl (aq)
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Second Tube
When the KSCN added into the solution the
pressure that given to equilibrium system is
additional concentration of SCN-
. Fe3+
ions reactwith SCN- that added, so the equilibrium move
to the left side and the color of solution become
darker.
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Third Tube
When the solution added by 2 mL of FeCl3,the color of solution will be darker because Fe 3+
ions from FeCl3 will move the equilibrium fromthe right to the left side.
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Fourth Tube
When 2 mL of Oxalic acid (H2C2O4) was added into solution. The
Oxalic acid ionized in water and form oxalic ion (C2O42-) which has
strongly bind with Fe3+ ions. The forming of stable ion [Fe(C2O
4)
3]3-
that has yellow color takes Fe3+ions in the solution, so the equilibrium
move from the left from the right side. The red color of solution will
change become yellow.
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When K2Cr
2O
7added by NaOH
Adding a base reduces the concentration of H2O+
ions in the solution, causing equilibrium to shift to
the left, or reactant side. This is demonstrated by thesolution becoming yellow.
H2O+
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Adding an acid will increase the
concentration of H2O+ ions in the equilibrium
system, forcing the equilibrium to shift to the
right, or product side. This is demonstrated by
the solution becoming orange
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Adding an acid will increase the
concentration of H2O
+
ions in the equilibriumsystem, forcing the equilibrium to shift to the
right, or product side. This is demonstrated by
the solution becoming orange
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Measure the liquid in graduated cylinder correctly (do not
parallax)
Use the same drop pipette to drop the additional liquid to the
solutionMake sure to stop dropping the liquid when it reach the
equilibrium point
Do not forget to calculate the dropping