Final answer:
The lower the L iso value, the stronger the electrolyte, due to factors such as acid strength, ion charge, and dissociation capacity. Strong acids like HCl and compounds like Ba(OH)2 display complete dissociation in water, indicating strong electrolyte properties.
Step-by-step explanation:
The lower the L iso value, the stronger the electrolyte. This relatedness between electrolyte strength and L iso value is connected to different factors, such as acid strength, ion charge, and lattice energy. The stronger an acid, the more readily it donates H+. An example is hydrochloric acid (HCl), which completely dissociates into its ions in aqueous solution, making it a strong electrolyte. Similarly, highly charged ions tend to ionize more, which also can indicate a strong electrolyte. Looking at compounds like Ba(OH)2 and HCl, we see they have high conductivity due to their ability to dissociate completely into ions.
Furthermore, there is a relationship between the strengths of a conjugate acid-base pair: the stronger the acid, the weaker its conjugate base, and vice versa. This means that in water, a strong acid like HCl will completely dissociate, becoming the strong electrolyte hydronium ion (the strongest acid that can exist in water), and its conjugate base will be comparatively weak. Factors influencing the strength of acids, like electronegativity of the central atom and its oxidation state, also play a role in this dissociation behavior, thus affecting electrolyte strength.