Which statement is true regarding weak acids in solution?

Weak acids in solution establish an equilibrium between the undissociated acid molecules and the ions produced when those acids partially dissociate. This is a defining characteristic of weak acids as opposed to strong acids, which completely dissociate in solution.

In a weak acid solution, the equilibrium can be represented by the general reaction:

HA ⇌ H⁺ + A⁻

Here, HA represents the weak acid, while H⁺ and A⁻ are the ions formed. The presence of the double arrow indicates that the reaction does not proceed to completion but rather reaches a state where the concentrations of the reactants and products remain constant. This equilibrium allows weak acids to have a relatively higher concentration of undissociated molecules compared to products in solution.

This property directly affects the conductivity of the solution, meaning weak acids can conduct electricity, but not as efficiently as strong acids due to the lower concentration of ions compared to fully dissociated solutions. Furthermore, weak acids typically have a pH lower than 7, indicating they are acidic; thus, the remaining options do not accurately describe the behavior of weak acids in solution.