Question

Consider the following equilibrium:

AgCl(s) Ag1+(aq) + Cl1-(aq)

Ho = 66 kJ

Use LeChatelier's principle to predict the effect on the chloride ion concentration caused by each of the following actions:

Action	Effect on [Cl1-]
adding silver chloride	---Select--- increases unchanged decreases
adding silver ion	---Select--- increases unchanged decreases
adding water	---Select--- increases unchanged decreases
heating	---Select--- increases unchanged decreases

Answer 1

AgCl(s) ------------------> Ag+(aq) + Cl-(aq)

adding silver chloride => here the AgCl is in solid form so when you add the solid to the equilibrium reaction there is no change in equilibrium position i.e not effected so no change in equilibrium shift

answer => Unchanged ( Cl- unchanged)

adding silver ion => here we are adding the aqueous form of the product i.e increasing the concentration of products so equilibrium shift to left i.e towards more reactant formation

answer => left (Cl- decreases )

adding water => i.e forming more ions then the reaction towards the more reactant formation i.e equilibrium shift to left

answer => left ( Cl- decreases)

heating => the delta H value is positive so it is endothermic reaction i.e heat is required for the product formation so when heating then more products are formed equilibrium shift to right

answer => right ( Cl- increases)