Answer: A net ionic equation for the neutralization of a weak acid with a strong base is:
Explanation:
- Let´s consider this balanced molecular equation:
HCN(aq) + NaOH(aq) --------} NaCN(aq) + H2O(l)
- You can see it is an acid-base reaction because OH (-) is taking away the H from HCN.
Where: NaOH(aq) is the base and
HCN(aq) is a weak acid as it has no oxygen.
- For the total ionic equation we will break up all the possible break ups and we get:
HCN(aq) + Na (+)(aq)+ OH(-) (aq) --------- } Na (+)(aq)+CN(-) (aq) + H2O(l)
- For the net ionic equation we reduce:
HCN(aq) + OH(-)(aq) -------- } CN(-)(aq) + H2O(l)
- We get the weak acid HCN(aq) plus the hidroxide ion which is the base.
The spectator ions is Na(+)
The net ionic equation for the reaction of any strong acid with any strong base is identical
Net ionic equations for acid-base reactions a neutralization reaction between a weak acid, HCN, and a strong base, KOH.
A weak acid, weak base reaction can be shown by the net ionic equation example:
HCl(aq) + NaOH(aq) ↔ H2O(l) + NaCl(aq) HF(aq) + OH-(aq) ↔ H2O(l) + F-(aq) HF(aq) + NaOH(aq) ↔ H2O(l) + NaF(aq) H3O+(aq) + OH-(aq) ↔ 2 H2O(l)
When a strong acid neutralizes a weak base, the resulting solution's pH will be less than 7.
Weak acids as hydrofluoric, HF only dissociate partially or will react with sodium hydroxide, NaOH , a strong base, to produce aqueous sodium fluoride, NaF , and water to get the net ionic equation that describes this neutralization reaction.
They are not considered to split apart into ions when writing net ionic equations.
This reaction is considered a neutralization reaction. The base (NaOH) and weak acid (CH3COOH) react to produce a salt (NaNO3 and water (H2O).
