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In the formation of the hydronium ion, what acts as the Lewis base?

Hydroxide

Explanation:

Under the Lewis definition, hydroxide goes about as the Lewis base, giving its electron pair to H+. Accordingly, in this adaptation of the balanced response, what intrigues us isn't the salt that structures, however the covalent bond that structures among Gracious and H+ to frame water.

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Although the hydronium ion is the nominal Lewis acid here, it does not itself accept an electron pair, but acts merely as the source of the proton that coordinates with the Lewis base Water, is an excellent example of a compound that can act as both Lewis acids (electron acceptor) and Lewis bases (electron donor). Ions such as the bicarbonate ion (HCO3-) and bisulfate ion (HSO4-) are also compounds that act as both Lewis acids and bases because they can either lose or gain electrons.

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*tilts head* sounds more like a statement

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.