Question

Which of the following reactions is properly classified as a precipitation, reduction/oxidation, and/or Bronsted-Lowry acid/base reaction? (1) CH3COOH(aq) + OH− (aq) → H2O(l) + CH3COO− (aq) is both precipitation and acid/base (2) CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) is both redox and acid/base (3) 2 H3O + (aq) + CaCO3(s) → Ca2+(aq) + CO2(g) + 3 H2O(l) is both redox and acid/base (4) 2 Na(s) + Cl2(g) → 2 NaCl(s) is both precipitation and redox (5) None of the above please explain why because i thought it would be A

Answer 1

(1) CH₃COOH (aq) + OH^- (aq) = H₂O (l) + CH₃COO^- (aq)

           This reaction is an acid base reaction but not a precipitation reaction as the products formed are highly soluble in water.

(2) CH₄ (g) + 2O₂ (g) = CO₂ (g) + 2H₂O (g)

         This reaction is a redox reaction but not an acid base reaction as there is no exchange of proton or electron pair.

(3) 2H₃O⁺ (aq) + CaCO₃ (s) = Ca²⁺ (aq) + CO₂ (g) + 3H₂O (l)

         This is an acid base reaction but not a redox as exchange of electron does not take place.

(4) 2Na (s) + Cl₂ (g) = 2NaCl (s)

         This reaction is a redox reaction as there is exchange of electron but as there is no liquid phase the question of precipitation does not arise.

So, None of the above classifications are correct.