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.

Conjugate acids and conjugate bases are the acids and bases that lose or gain protons. NH4+ is the conjugate acid to the base NH3, because NH3 gained a hydrogen ion to form NH4+.The conjugate base of an acid is formed when the acid donates a proton.

2015年11月12日 · The conjugate base of an acid, any acid, is defined as the acid "LESS" a proton, H^+. The conjugate acid of a base, any base, is defined as the base "PLUS" a proton. Phosphoric acid, H_3PO_4, is the parent acid. If it loses a proton, H^+, we conserve both mass and charge, and H_2PO_4^- results. And what is the conjugate base of this beasty? Again, …

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.

2015年11月29日 · The conjugate acid of any species, is that species plus a proton; so it's H_2PO_4^(-). When we add a proton, we must conserve both mass and charge, we add H^+ to HPO_4^(2-) so the conjugate acid is simply H_2PO_4^(-).

2015年11月5日 · dihydrogen phosphate dihydrogen (because there are 2 H atoms) plus the phosphate ion (PO_4^"3-"). There are a few rules that one must obey in naming polyatomic ions, but it all can get confusing sometimes that most students are reduced to just memorizing the names and chemical symbols for all common cations and anions (both monoatomic and …

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

$\ce{HPO4^-{2}}$ 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8月25日 · Simply add or substract a proton from H_3PO_4. Phosphoric acid is the parent acid, i.e. H_3PO_4. Remove a proton from this, we get, H_2PO_4^- as the conjugate base. Or rather phosphoric acid donates a proton to water to give H_3O^+ and H_2PO_4^-. And remove a proton from H_2PO_4^- to get HPO_4^(2-) as the conjugate base. In water that's about as far …

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).