Why is the Hydrogen Phosphate Ion HPO4-2? exactly how does the happen? The Hydrogen Ion is H+1 and also the Phosphate Ion is (PO4)-3. Shouldn't it it is in H3(PO4)? WolframAlpha perform both here: http://www.wolframalpha.com/input/?i=Hydrogen+ion+%2B+Phospate+ion


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H*3PO4* is no an ion, it is phosphoric acid. To be thought about an ion a molecule must have a charge. Friend can also have dihydrogen phosphate, i beg your pardon is H*2PO4*-1.

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H3PO4 is a multiprotic acid. This means that as soon as it dissolves, the dissolves more than once, yielding more than one proton, or H+ ion. The an initial dissociation in water is: H3PO4 -> H+ + H2PO4- The 2nd dissociation is: H2PO4- -> H+ + HPO42- The final dissociation is: HPO42- -> H+ + PO43-. For this reason hydrogen phosphate has actually a charge of 2- because two positively charged hydrogens were removed by dissociation in water.

I apologize for the formatting, or lack thereof. Hope you have the right to still understand what i was trying to convey.


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level 1
· 7y

One other thing to keep in mind:

H3PO4 == Phosphoric acid

H2PO4(-) == Phosphorous acid (and generally has a counter cation for the full, neutral molecule)

HPO4(2-) == Hydrogen Phosphate. When technically the tertiary acid of phosphorIC acid, and the conjugate base of phosphorOUS acid, it's more-properly called hydrogen phosphate fairly than something v the 'acid' label due to the fact that it's basic (rather than acidic).

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Hydrogen Phosphate is HPO4(2-) due to the fact that in physics form, it will have counter-cations come balance the charge (like sodium, making that Na2HPO4 as a solid--but when it dissolves, the sodiums dissociate, leaving HPO4-)


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level 2
Op · 7y

Thank you. I type of get it now. Why then do other ions that incorporate don't perform this? Is it just hydrogen?


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