Final answer:
Synthesis and decomposition are not types of neutralization reactions; the first involves combining substances, while the second involves breaking down a compound into multiple products. Neutralization reactions, however, involve the reaction of an acid and a base to form water and a salt.
Step-by-step explanation:
No, synthesis and decomposition are not both neutralization reactions. A synthesis reaction is when multiple reactants combine to form a single product. An example is:
Fe₂O₃ + 3 SO₃ → Fe₂(SO₄)₃
This is considered a synthesis reaction as multiple reactants (iron(III) oxide and sulfur trioxide) react to form one product (iron(III) sulfate).
In contrast, a decomposition reaction is when a single compound breaks down into two or more substances. For example:
(NH₄)₂Cr₂O₇ → Cr₂O₃ + 4H₂O + N₂
This corresponds to a decomposition reaction because one single compound (ammonium dichromate) decomposes to form various different substances (chromium(III) oxide, water, and nitrogen gas).
A neutralization reaction is specifically an acid-base reaction where an acid and a base react to form water and a salt. For instance:
H₂SO₄ (aq) + Sr(OH)₂ (aq) → 2 H₂O(l) + SrSO₄ (aq)
This reaction between sulfuric acid and strontium hydroxide is a neutralization reaction, resulting in the formation of water and the salt strontium sulfate. Neutralization reactions can also occur when one reactant is not soluble, such as in the reaction of hydrochloric acid with iron(III) hydroxide:
3 HCl(aq) + Fe(OH)₃ (s) → 3 H₂O(l) + FeCl₃ (aq)
This also results in water and a salt (iron(III) chloride), demonstrating the utility of neutralization reactions in practical applications like removing rust stains.