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So I understand when finding net ionic equations, you have to consider whether a

ID: 474504 • Letter: S

Question

So I understand when finding net ionic equations, you have to consider whether a compound with dissociate or not. You don't break up weak acids,weak bases, molecualr compounds and insouble compounds. For example I know HF and HNO2 are weak acids. And if I saw them in the equation...I would not break them up because they don't fully dissociate. As well as CH3COOH (acetic acid, week acid). However, if the equation included Ba(CH3COO)2 (barium acetate)...would I break up Barium acetate. That compound contains a weak acid. Is it considered a weak acid that does not fully dissociate? I thought I would but I have had probles where you do break them up. For example...Barium acetate + ammonium. The net ionic equation is Ba+2 + SO4-2 ---BaSO4(s). I hope my exaple makes sense.

Explanation / Answer

Note first thing that weak and strong acids both dissociate but the important thing is that degree of dissociation or what quantity dissociation takes place.

weak acids are weak electrolyte and they dissociates partially ( degree of dissociation is less )

but

strong acid or salts dissociates completely ( degrre of dissociation is = 1.0 )

and

Ba(CH3COO)2 and (NH4)2SO4 both are strong electrolyte and dissociates completely.

therefore

Ba(CH3COO)2 (aq) + (NH4)2SO4 (aq) -------------> BaSO4 (s) + 2 CH3COONH4 (aq)

or

Ba+2 + SO4-2 ------> BaSO4(s)

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