What is the net ionic equation for the reaction of acetic acid, CH3COOH, with NH3?

A. CH3COOH(aq) + NH3(aq)→NH4+ + CH3COO– (aq)

B. CH3COOH(aq) + NH3(aq)→NH4CH3COO(aq)

C. CH3COO– (aq)+ H+ (aq) + NH3(aq)→NH4CH3COO(aq)

D. H+ (aq) + NH3(aq)→NH4+ (aq)

E. H+ (aq) + OH– (aq)→H2O(aq)


answeredMar 15, 2019by Anjal(76.9k points)selectedMar 16, 2019by faiz

Correct option (A)CH3COOH(aq) + NH3(aq)→NH4++ CH3COO–(aq)

Explanation:

Begin by looking at the reactants and determining their dissociation abilities. Acetic acid is a weak acid, therefore, it should be written in the reaction as HC2H3O2(aq) to show that it is dissolved but not fully dissociated. Ammonia is a weak base in solution that also doesn’t have any ions. It must be written as a dissolved molecule, NH3(aq), as well. Next, consider the products. The proton from acetic acid should be moved to the ammonia molecule, making the ionic equation:

HC2H3O2(aq) + NH3(aq) → C2H3O2 – + NH4+

Turning this into a net ionic equation means not doing anything; there are no spectators. Now choose from the responses.

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