Question

write the word equation form of the net ionic equation for all neutralization equations.

Answer 1

@xxfreshboy , you supposed to give the equations , right ?

Answer 2

im confuzed what do you mean im supposed to write like word equations i believe.

Answer 3

@shivam_bhalla

Answer 4

all neutralizations produce the same 2 things: some kind of salt and water. The exact formula of the sale doesn't matter, since it will be soluble and dissociated in solution anyway. The net ionic reaction of all neutralizations will be the reation that forms water from H+ and OH-.

Answer 5

See

sodium hydroxide+ hydrochloric acid --> sodium choride + water

Answer 6

*chloride

Answer 7

@JFraser: does xxfreshboy's question implicitly mean only strong acids and bases are concerned? I am asking because of the last sentence you wrote.

Answer 8

@Vincent-Lyon.Fr all bases produce hydroxide ions, whether they have one in their formula or not. For Example:\[NH_3(aq) + H_2O \leftrightharpoons NH_4^{+1} + OH^{-1}\] even though the NH3 has no hydroxide, it produces a hydroxide when it dissociates in water. The general form of all neutralizations is the same, regardless of strong acid\strong base, or weak acid\weak base

Answer 9

I was reasoning within Bronsted's theory, so I did not agree with the word "net" in your answer, as H+ and OH- have to be produced by other reaction with water.
When reacting a weak acid with a weak base, no water is formed.

Answer 10

I would argue that WA\WB neutralizations do produce water, just very little of it based on small Ka\Kb values.

Answer 11

Maybe, but the "net" equation is:
\[CH _{3} COOH+NH _{3} \rightarrow CH _{3} COO ^{-}+NH _{4} ^{+}\]

Answer 12

and no water appears anywhere in it.
I guess the expected answer implied worlking within Arrhenius' context.

Answer 13

I think you're mixing up two reactions, Vincent:

(1) Acid dissociation, either HCl(aq) + H2O(l) = H3O+(aq) + Cl-(aq) for a strong acid, or HOAc(aq) + H2O(l) = H3O+(aq) + OAC-(aq) for a weak.

(2) Neutralization, which is, as JFraser says, always simply H3O+(aq) + OH-(aq) = 2H2O(l)

I agree to some extent this is a question of arbitrary viewpoint, since there's not necessarily an easy bright line distinction we can make between looking at the reactions in this "two step" way and looking at it in the overall way you are taking. But as a matter of empirical fact, the two-step approach is how we look at it traditionally. In part this is because a more sophisticated viewpoint (than is usually taught in gen chem) suggests we want to emphasize the very important role of water in these reactions. So we separate out the attack of water on the acid in the first step.

I should add that there are probably reactions that occur in the gas phase that can both be characterized as acid-base (at least in the Lewis sense) and which do not involve water at all.

Answer 14

It's a matter of definitions and you know better than me what is expected in these rather sibylline questions!

xxfreshboy's question went: "write the word equation form of the NET ionic equation for all neutralization equations."

So I assumed you should not simply write PART but ALL of the overall process from what you put in water to what you get as end-products.
I simply mean separating in different steps seems to go against the requirement to write a NET equation.

Excluding the case Wa/Wb, but valid for all other cases Sa/Wb, Wa/Sb and Sa/Sb, I would write:
acid + base -> water + salt

Answer 15

Yes, but what I'm saying is that "neutralization" is usually defined to be what happens after the acid and water, and base and water, separately, have come to equilibrium.

Imagine, if you will, mixing your HOAc and water in one beaker and allowing to come to equilibrium. Now mix your NH3 and water in another. Both will react with water, producing H3O+ and OAc- in one and NH4+ and OH- in the other. Now magically instantaneously mix them. This is the neutralization step, and what happens is that the previously generated H3O+ and OH- react. The NH4+ and OAc- do not.

Now in an actual beaker in an actual lab, what happens is much more complicated, and all of the interesting reactions are going on at once, so the true situation is much more muddled. But for teaching purposes we tend to pretend we can cleanly separate the steps as I've described above.

This is not to say I think you are wrong in anything you say. There's nothing wrong with regarded the whole reaction, from a bottle of HOAc and tank of NH3 through to the end, as the neutralization reaction. Some people might even do that. I'm just saying I think it's a minority viewpoint, and that's so simply because we usually want to emphasize the role of water in the overall process.