Final answer:
Reactions (a), (b), and (c) from the first set are acid-base reactions, whereas (d) is a precipitation reaction and (e) is an oxidation-reduction reaction. For question 19, all reactions (a), (b), and (c) are classified as oxidation-reduction reactions.
Step-by-step explanation:
To identify which of the provided reactions are acid-base reactions and which are oxidation-reduction reactions, let's analyze each one:
(a) HCOOH(aq) + NaOH(aq) → HCOONa(aq) + H2O(l) is an acid-base reaction because it involves a transfer of a proton (H+) from formic acid (HCOOH) to the base sodium hydroxide (NaOH), resulting in the production of water (H2O) and a salt (HCOONa).
(b) HI(aq) + CH3NH2(aq) → CH3NH3+(aq) + I-(aq) is an acid-base reaction where hydroiodic acid (HI) donates a proton to the base methylamine (CH3NH2), forming methylammonium ion (CH3NH3+) and iodide ion (I-).
(c) NaOH(aq) + HCIO4(aq) → NaClO4(aq) + H2O(l) is also an acid-base reaction as it involves sodium hydroxide, a strong base, reacting with perchloric acid, a strong acid, to form a salt (NaClO4) and water.
(d) and (e) are not acid-base reactions. (d) 2 NaCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 NaNO3(aq) is a precipitation reaction, and (e) Fe3+(aq) + 3 Ag(s) → 3Ag+(aq) + Fe(s) is an oxidation-reduction reaction as there is a transfer of electrons between silver (Ag) and iron (Fe).
All the reactions in question 19 are oxidation-reduction reactions:
- (a) Na2S(aq) + 2HCl(aq) → 2NaCl(aq) + H₂ S(g)
- (b) 2Na(s) + 2HCl(aq) → 2NaCl(aq) + H₂(g)
- (c) Mg(s) + Cl₂ (g) → MgCl₂ (s)