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Need help with net ionic equation for weak acid/base neutralization.

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Aqueous acetic acid is neutralized by aqueous barium hydroxide.
\[Ba(OH)_{2}(aq)+2CH _{3}OOH(aq) \rightarrow 2H _{2}O(l)+Ba(CH _{3}OO)_{2}(aq)\]
that is the balanced equation

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Other answers:

\[Ba ^{2+}(aq)+2OH ^{-}(aq)+2H ^{+}(aq)+2CH _{3}OO ^{-}(aq)\rightarrow2H _{2}O(l)+Ba(CH _{3}OO)_{2}(aq)\]
chould be the balanced ionic equation
Getting rid of the spectator ions should leave 2H and 2OH
\[H ^{+}(aq)+OH ^{-}(aq)\rightarrow H _{2}O(l)\]
but I am told by mastering chemistry, "This is not the expected net ionic reaction when the reaction involves a weak acid such as acetic acid."
So I tried \[CH _{3}OOH(aq)+OH ^{-}(aq)\rightarrow H _{2}O(l)+CH _{3}OO ^{-}(aq)\]
Still wrongaccording to mastering chemistry
I believe it is: \[CH_3OOH(aq) + H_2O (l) \rightarrow H_3O^+ (aq)+ CH_3OO^- (aq)\]

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