Would it be correct to say that it is harder for a weak electrolyte to dissociate in a solution than it is for a stronger electrolyte to dissociate? If a weak electrolyte can't dissociate completely it wouldn't be able to form an equilibrium reaction right?
yes
Second question: No Equilibrium does not depend on complete dissociation. At equilibrium, the rate of dissociation is equal to the rate of reassociation.
To determine if it is harder for a weak electrolyte to dissociate in a solution compared to a stronger electrolyte, you can look at the dissociation constants. The dissociation constant, usually represented as K, is a measure of how readily a substance dissociates in a solution.
A strong electrolyte, such as a strong acid or a soluble ionic compound, completely dissociates into ions in a solution. This means that the concentration of ions in the solution is high, resulting in a high dissociation constant (K).
On the other hand, a weak electrolyte only partially dissociates in a solution. This means that the concentration of ions is lower compared to a strong electrolyte. As a result, the dissociation constant (K) for a weak electrolyte is lower than that of a strong electrolyte.
Therefore, it can be said that it is generally harder for a weak electrolyte to dissociate completely in a solution compared to a stronger electrolyte.
Regarding the second question, it is true that equilibrium does not depend on complete dissociation. In an equilibrium reaction, the rate of dissociation is equal to the rate of reassociation. This means that even if a weak electrolyte only partially dissociates, an equilibrium can still be established between the dissociated and undissociated molecules. The extent of dissociation depends on the reaction conditions and the properties of the weak electrolyte.
In summary, a weak electrolyte may not dissociate completely in a solution, but it can still form an equilibrium reaction with both the dissociated and undissociated forms present.