Final answer:
Soluble solutes such as HCl, NaOH, and HNO3 are classified as strong electrolytes because they completely dissociate into ions, HC2H3O2 and HF are weak electrolytes as they only partially dissociate, and C2H5OH and C6H12O6 are nonelectrolytes because they do not form ions in solution.
Step-by-step explanation:
Electrolyte Classification of Soluble Solutes
To classify each soluble solute as a strong electrolyte, weak electrolyte, or nonelectrolyte, we must understand their behavior when dissolved in water:
HCl (hydrochloric acid) and NaOH (sodium hydroxide) completely dissociate into ions in aqueous solutions, which qualifies them as strong electrolytes.
HC2H3O2 (acetic acid) and HF (hydrofluoric acid) partially dissociate into ions, which makes them weak electrolytes.
C2H5OH (ethanol) and C6H12O6 (glucose) do not dissociate into ions; rather, they dissolve into individual neutral molecules, making them nonelectrolytes.
HNO3 (nitric acid) is a strong acid that fully dissociates in water, so it is a strong electrolyte as well.
Understanding the extent to which these substances dissociate in water into ions is crucial for determining their classification. Ionic compounds like HCl and NaOH are strong electrolytes. Acids such as HC2H3O2 and HF, which do not dissociate completely, are weak electrolytes. Ethanol and glucose are examples of nonelectrolytes because they do not contribute ions to their solutions.