Which statement most accurately differentiates strong electrolytes and weak electrolytes?

• A. Strong electrolytes do not dissociate in solution.
• B. Weak electrolytes fully dissociate; strong electrolytes partially dissociate.
• C. Strong electrolytes fully dissociate in solution; weak electrolytes only partially dissociate; Examples include NaCl and HCl for strong; CH3COOH for weak.
• D. Electrolyte strength depends on temperature; not on dissociation.

Answer: (C)

The key idea is how much a substance Ionizes in solution. Electrolytes conduct electricity because they form ions in water, and the strength classification depends on the extent of that ionization. Strong electrolytes dissociate completely, producing a large number of ions and thus high conductivity. Weak electrolytes dissociate only partially, so only a fraction of molecules becomes ions, leading to fewer charge carriers and much lower conductivity. That’s why NaCl and HCl are described as strong electrolytes—they largely separate into ions in solution. CH3COOH is a classic weak electrolyte because it only partly ionizes to give some acetate and hydrogen ions, with most remaining as undissociated acetic acid molecules. The statement that strong electrolytes do not dissociate contradicts the fundamental reason electrolytes conduct electricity. The claim that strong electrolytes fully dissociate while weak ones partially dissociate is exactly what defines the difference. Temperature can influence the degree of dissociation, but the defining factor is the extent of ionization in solution, not temperature alone.