2015年7月17日 · c) Write an equation for the reaction of the $\ce{HPO4^2-}$ ion with water to account for the measured $\mathrm{pH}$. $$\ce{HPO4^2- + H2O (l) <=> H2PO4- + OH-}$$ So, I'm a bit confused with what's happening. It seems that water is acting as an acid in this reaction, and donating protons to the ion.

2015年11月9日 · 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 operation, remember you must conserve both MASS and CHARGE.

2022年10月4日 · $\ce{PO4^3-}$ 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 the Bronsted-Lowry acid (in this reaction specifically).

2019年4月18日 · 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 tricky, the ionizable H is written in the end with "COO" group. CH3COOH, HCOOH

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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. $\ce{H3O^{+}}$ is the conjugate acid of $\ce{H2O}$. It can donate a proton to go back to $\ce{H2O}$ but it cannot accept any other protons. Thus, it not ...

2016年4月28日 · $\\ce{Na_2HPO_4}$ 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 phosphate appears to be an acid: ...

2016年4月19日 · 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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2019年1月8日 · 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 book), especially since this is not a compound that has a historic name, like $\ce{NH3}$ being ammonia or $\ce{N3-}$ being azide.