Asked by ny
Comparing Strong and Weak Acids and Bases
Which will become completely dissociated when dissolved in water?
All Answers 1
Answered by
GPT-5 mini
AI
Strong acids and strong bases.
- Strong acids (e.g., HCl, HBr, HI, HNO3, HClO4, and the first proton of H2SO4) essentially fully dissociate in water:
HCl → H+ + Cl−
- Strong bases (e.g., alkali metal hydroxides like NaOH, KOH; Ba(OH)2 is also a strong base in solution) likewise nearly completely dissociate:
NaOH → Na+ + OH−
Weak acids (acetic acid, HF, H2CO3, etc.) and weak bases (NH3, many amines) only partially dissociate; an equilibrium exists between the undissociated and dissociated forms (characterized by Ka or Kb).
Note: “Completely” is a practical simplification — dissociation is so near 100% for strong species under normal conditions that they are treated as fully dissociated.
- Strong acids (e.g., HCl, HBr, HI, HNO3, HClO4, and the first proton of H2SO4) essentially fully dissociate in water:
HCl → H+ + Cl−
- Strong bases (e.g., alkali metal hydroxides like NaOH, KOH; Ba(OH)2 is also a strong base in solution) likewise nearly completely dissociate:
NaOH → Na+ + OH−
Weak acids (acetic acid, HF, H2CO3, etc.) and weak bases (NH3, many amines) only partially dissociate; an equilibrium exists between the undissociated and dissociated forms (characterized by Ka or Kb).
Note: “Completely” is a practical simplification — dissociation is so near 100% for strong species under normal conditions that they are treated as fully dissociated.
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.