Chemistry · Ionic Equilibrium
Different acid-base theories help explain chemical behavior. Arrhenius acids give H+ in water, while Bronsted acids donate protons and form conjugate bases. Lewis acids accept electron pairs. A buffer solution resists pH change and its pH can be calculated using the Henderson-Hasselbalch equation. The common ion effect reduces solubility of salts and is involved in Ksp calculations. For weak acids and bases, Ka × Kb = Kw. Which of the following statements are correct? (A) Lewis base is a proton donor. (B) Solubility of BaSO4 decreases in presence of SO42− ions. (C) NH3 is a Bronsted base and accepts a proton. (D) Buffer solution shows a large pH change with small acid/base addition.
Verified Solution4 OptionsUpdated: October 2026👁️1 View
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- 1(A), (B), and (C)
- 2(A), (C), and (D)
- 3(B), (C), and (D)
- 4(B) and (C) only✓
Correct answer
(B) and (C) only
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