What is the net ionic equation for CH3COOH reacting with NaOH?
In terms of NET ionic equation, things get a little tricky. ChemWiz's previous answer would be correct for a strong acid, strong base reaction (as in HCl + NaOH). However, for a weak acid like acetic acid (CH3COOH), things are a little different because it does not completely disassociate (ionize) in water, as does HCl. However, NaOH, being a strong base, does completely ionize in water. So, the general reaction should look more like this:
CH3COOH + Na+ + OH- ==> CH3COO- + Na+ + H2O
Noticing that the Na+ ion is a 'spectator ion,' and, therefore, not involved in the net reaction (imagine it remaining dissolved in the water, not being directly involved in the reaction process). Therefore, the NET IONIC REACTION is as follows:
CH3COOH + OH- ==> CH3COO- + H2O
Also, make sure not to forget the respected charges on the ions!! They are an integral part of the net ionic equation! =)
You should easily be able to figure this out. Acetic acid is monoprotic (1 acidic proton). Sodium hydroxide is monobasic (1 OH); the proportions are 1:1
CH3COOH + NaOH => CH3COONa + H2O
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