Answer:
This question is incomplete but the completed question is below
Which net ionic equation best represents a weak acid-strong base reaction?
(a) H₃BO₃ (aq) → BO₃⁻ (aq) + H₂O (l)
(b) 2 OH⁻ (aq) → H₂O (l)
(c) H₃BO₃ (aq) + OH− (aq) → BO₃− (aq) + H₂O (l)
(d) H₃BO₃ (aq) + KOH (aq) → KBO₃ (aq) + H₂O (l)
The correct option is c
Explanation:
The reaction between an acid and a base is called neutralization reaction. Neutralization reaction is the reaction between an acid and a base to produce salt and water. Here, the metal from the base dissociates (leaving OH⁻) and binds to the non-metal in the acid which forms the salt (in the product). When the acid dissociates, the hydrogen ion (H⁺) from the acid binds with the hydroxyl group (OH⁻) of the base to form water.
A strong acid is an acid that dissociates completely in water (example is HCl) while a weak acid dissociates partially in water (example is H₃BO₃). Similarly, a strong base is a base that dissociates completely in water (example is NaOH) while a weak base is a base that dissociates partially in water (NH₃).
From the above explanation, it can be deduced that the correct option is c because H₃BO₃ (boric acid) dissociates to form hydroxyl ion (H⁺) and borate ion (BO₃³⁻) as shown below
H₃BO₃ → H⁺ + BO₃³⁻
This H⁺ (in the product) ionically reacts with the OH⁻ to form H₂O hence the complete/net ionic equation is
H₃BO₃ + OH⁻ → BO₃⁻ + H₂O
