Question

An aqueous solution is made by mixing 5.1 mL of 0.40 M Co(NO₃)₂ and 7.9 mL of 12.0 M HCl, and the following is the equilibrium reaction that takes place.

[Co(H₂O)₆]²⁺(aq) + 4Cl^- (aq) <-----> [CoCl₄]^2- (aq) + 6H₂O(l)

Assuming the above reaction is exothermic in the forward direction (toward the product side), predict whether the following statements (in relation to the above equilibrium reaction in aqueous solution) are "True" or "False".

Addition of H₂O causes the equilibrium to shift to the left (reactant side).
Heating does not cause the equilibrium to shift to either side, it only speeds up the reaction.
Addition of HCl causes the equilibrium to shift to the left (reactant side).
In the ddition of HCl, equilibrium will not be shifted to either side because H⁺ ions (from HCl) react with NO₃^- (from cobalt (II) nitrate) and form HNO₃.
The above equilibrium reaction has a negative enthalpy change in the reverse direction (toward the reactant side).

Answer 1