We have a volume $[H_3PO_4]-=2.0*N$ . If this is to be reacted with an EQUAL volume of sodium hydroxide...what concentration with respect to $[NaOH]$ is required?

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Answer 1 · 2017-09-01T06:07:32

Well, its $4*N$ ...........

Phosphoric acid acts as a diacid in aqueous solution....

$H_3PO_4(aq) + 2NaOH(aq) rarr Na_2HPO_4(aq) + 2H_2O(l)$

And so if you got $[H_3PO_4]=2*mol*L^-1$ , this is $4*N$ with respect to $H_3O^+$ . The volume is irrelevant.

We have a volume [H_3PO_4]-=2.0*N[H_3PO_4]-=2.0*N. If this is to be reacted with an EQUAL volume of sodium hydroxide...what concentration with respect to [NaOH][NaOH] is required?