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 $\mathrm{pH}$. $$\ce{HPO4^2- + H2O (l) <=> H2PO4- + OH-}$$ …

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 …

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. …

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^+ …

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 …

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 …

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 …

$\ce{HPO4^-{2}}$ 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. …

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 …

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 …