Chapter 4
Q. 4.4
Write a net ionic equation for each of the following reactions in dilute water solution.
(a) Hypochlorous acid (HClO) and calcium hydroxide.
(b) Ammonia with perchloric acid (HClO_{4}).
(c) Hydriodic acid (HI) with sodium hydroxide.
STRATEGY
1. Determine the nature of the compound (acid or base; strong or weak) and its reacting species. (Table 4.1 and Figure 4.8 are helpful.)
2. Recall Table 4.2 and write a net ionic equation for the acid-base reaction.
Table 4.1 Common Strong Acids and Bases
| Name of Base | Base | Name of Acid | Acid |
| Lithium hydroxide | LiOH | Hydrochloric acid | HCl |
| Sodium hydroxide | NaOH | Hydrobromic acid | HBr |
| Potassium hydroxide | KOH | Hydriodic acid | HI |
| Calcium hydroxide | Ca(OH)_{2} | Nitric acid | HNO_{3} |
| Strontium hydroxide | Sr(OH)_{2} | Perchloric acid | HClO_{4} |
| Barium hydroxide | Ba(OH)_{2} | Sulfuric acid | H_{2}SO_{4} |
Table 4.2 Types of Acid-Base Reactions
| Net Ionic Equation | Reacting Species | Reactants |
| H^{+}(aq) + OH^{-}(aq) → H_{2}O | H^{+}–OH^{-} | Strong acid–strong base |
| HB(aq) + OH^{-}(aq) → H_{2}O + B^{-}(aq) | HB–OH^{-} | Weak acid–strong base |
| H^{+}(aq) + B(aq) → BH^{+}(aq) | H^{+}–B | Strong acid–weak base |
Step-by-Step
Verified Solution
| HClO: weak acid; Ca(OH)_{2}: strong base
For HClO: HClO; for Ca(OH)_{2}: OH^{-} HClO(aq) + OH^{-}(aq) → ClO^{-}(aq) + H_{2}O |
(a) Nature of the compounds reacting species net ionic equation |
| HClO_{4}: strong acid; NH_{3}: weak base
For HClO_{4}: H^{+}; for NH_{3}: NH_{3} H^{+}(aq) +NH_{3}(aq)→ NH_{4}^{+}(aq) |
(b) Nature of the compounds reacting species net ionic equation |
| HI: strong acid; NaOH: strong base
For HI: H^{+} ; for NaOH: OH^{-} H^{+}(aq) + OH^{-}(aq) → H_{2}O |
(c) Nature of the compounds reacting species net ionic equation |