If you add more ammonia, NH3(a q), to the equilibrium mixture described by the chemical equation

step 1 Let's start with this equilibrium mixture. We have C .U. N .H .3. 6 .2 plus aqueous. That's in e

If you add more ammonia, NH3(a q), to the equilibrium...

If you add more ammonia, $\mathrm{NH}_{3}(a q),$ to the equilibrium mixture described by the chemical equation given below, what will happen? Explain your thinking. $$ \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{6}^{2+}(a q) \leftrightharpoons \mathrm{Cu}^{2+}(a q)+6 \mathrm{NH}_{3}(a q) $$

If you add more ammonia, $\mathrm{NH}_{3}(a q),$ to the equilibrium mixture described by the chemical equation given below, what will happen? Explain your thinking.
$$
\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{6}^{2+}(a q) \leftrightharpoons \mathrm{Cu}^{2+}(a q)+6 \mathrm{NH}_{3}(a q)
$$

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Key Concepts

Le Chatelier's Principle

This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system adjusts itself to partially counteract the change and a new equilibrium is established. When an additional reactant or product is added, the equilibrium shifts in the direction that tends to reduce that change.

Chemical Equilibrium

Chemical equilibrium is the state in which the forward and reverse reactions occur at the same rate, so there is no net change in the concentration of reactants and products. Changes in concentration, temperature, or pressure can disturb this balance, causing the system to shift and re-establish equilibrium.

Stoichiometry in Equilibrium Reactions

The stoichiometric relationships in a balanced chemical equation determine how the concentrations of reactants and products are affected by a shift in equilibrium. When a component is added or removed, the proportions dictated by the reaction stoichiometry guide the new equilibrium configuration to offset the disturbance.

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