Question

what type of compound is represented by the graph?
consider how much ha breaks into its ions.
strong acid
weak acid
weak base
strong base

Explanation:

Step1: Analyze strong acid dissociation

A strong acid dissociates completely in water. So if HA were a strong acid, after adding to water, there would be almost no HA left, only \(H^{+}\) and \(A^{-}\). But the graph shows some HA still present.

Step2: Analyze weak acid dissociation

A weak acid dissociates partially in water. The reaction \(HA
ightleftharpoons H^{+}+A^{-}\) is in equilibrium. So there will be a significant amount of HA along with \(H^{+}\) and \(A^{-}\) ions, which matches the graph.

Step3: Analyze base cases

Bases produce \(OH^{-}\) (for Arrhenius bases) or accept \(H^{+}\) (for Bronsted - Lowry bases). The graph shows \(H^{+}\) and \(A^{-}\) (not \(OH^{-}\) related species in a simple sense for the given notation), so it is not a base (neither weak nor strong).

Answer:

weak acid