Use Le Châtelier’s Principle to predict how the four equilibrium systems will re

Question

Use Le Châtelier’s Principle to predict how the four equilibrium systems will respond to the changes you will make:

I.       CH3COOH (aq)   CH3COO– (aq) + H+ (aq)

How will adding sodium acetate (CH3COONa) initially change [CH3COOH], [CH3COO–], and [H+]? How should the equilibrium system respond to this change?

II.     Fe3+ (aq) + SCN– (aq)   FeSCN2+ (aq)

1.   How will adding potassium thiocyanate (KSCN) initially change [Fe3+], [SCN–], and [FeSCN2+]? How should the equilibrium system respond to this change?

2.   How will adding silver nitrate (AgNO3) initially change [Fe3+], [SCN–], and [FeSCN2+]? How should the equilibrium system respond to this change?

III.    Co2+ (aq) + 4 Cl– (aq)   CoCl42– (aq)

How will diluting with water initially change [Co2+], [Cl–], and [CoCl42–]? How should the equilibrium system respond to this change?

IV.    CO2 (aq and g) + H2O (l)   H+ (aq) + HCO3– (aq)

How should the equilibrium system respond when the pressure is lowered?

Explanation / Answer

There are multiple questions here. I am allowed to answer only 1 at a time. So I will answer question 1st 2 for you.
I) CH3COONa   ---> CH3COO- + Na+
CH3COOH <---> CH3COO- + H+
So increasing CH3COO- will shift the reaction in backward direction.
so CH3COOH will incraese
CH3COO- will decrease
H+ will decrease

II)
1.
KSCN ---> K+ + SCN-
Adding KSCN will make the reaction go in forward direction.
Fe3+ decreases
SCN- decreases
FeSCN2+ incraeses
2.
AgNO3 don't have any common ion. SO it will no effect equilibrium.

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