Equilibrium/Le Chatelier's PrincipleWatch
But when a different substance is added, for example,
CoCl42- (aq) + 6H2O (l) <---> Co(H2O)62+ (aq) + 4Cl- (aq)
has AgNO3(aq) added to it, the system shifts in favour of the products.
Can someone please explain to me why this happens?
The Ag+ will react with the Cl- decreasing the concentration of Cl-, so the equilibrum will shift to the right
I have one more quick question, along the same lines.
H+ (aq) + HTb- (aq) <----> H2Tb (aq)
HTb- (aq) <---> H+ (aq) + Tb2- (aq)
When HCl is added to the first reaction, there is an increase in the amount of H+, so the system shifts to the left and turns red. When NaOH is added to the same solution (the red solution) it turns blue. How would I describe this and why does this happen?
The yellow is the reactants and the blue the products for the second one.