Jul 17, 2015 · c) Write an equation for the reaction of the $\ce{HPO4^2-}$ ion with water to account for the measured $\mathrm{pH}$. $$\ce{HPO4^2- + H2O (l) <=> H2PO4- + OH-}$$ …

Nov 9, 2015 · The conjugate base of a species is simply the acid less a H^+ species. So what is the creature we get when we take H^+ from biphosphate ion, HPO_4^(2-). When you do this …

Oct 4, 2022 · $\ce{PO4^3-}$ and $\ce{HPO4^2-}$ are in fact conjugate acid/base pairs. However, the question doesn't ask for that. However, the question doesn't ask for that. Rather it asks for …

Apr 18, 2019 · If you see, HPO4 (2-), you should be able to guess that HPO4(2-) can accept one or two proton(s), however it can also lose the last one. For small organic ions, it is slightly …

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$\ce{HPO4^-{2}}$ is the conjugate base of $\ce{H2PO4^{-}}$. It can accept a proton to go back to $\ce{H2PO4^{-}}$ or it can donate a proton to become $\ce{PO4^{-3}}$. Thus, it is amphoteric. …

Apr 28, 2016 · $\\ce{Na_2HPO_4}$ is amphoteric, which means it can act as a base or as a acid depending on which substance they react with. This is the reaction in which disodium …

Apr 19, 2016 · How to calculate pH of a solution when $\ce{H3PO4}$, $\ce{NaH2PO4}$, $\ce{Na2HPO4}$ and $\ce{Na3PO4}$ are mixed together in certain amounts to form a solution?

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Jan 8, 2019 · First of all, I am aware of this question.The purpose of my question is to understand why people seem to break the rules that IUPAC has set (See example five on page 76 of the …