2012年8月27日 · It is much easier to explain it on a simpler example – the $\ce{O3}$ molecule. It has the structure of resonance hybrid of $\ce{O=O+-O-}$ and its mirror.

2021年6月17日 · In spite of the viscosity of the acid, the effective conductivities of the $\ce{H3SO4+}$ and $\ce{HSO4-}$ ions are high due to an intramolecular proton-switch mechanism (analogous to the Grotthuss mechanism in water), making sulfuric acid a good conductor of electricity. It is also an excellent solvent for many reactions.

2024年12月14日 · H3SO4+ is obviously much stronger acid than $\ce{H2SO4}$, but is just minor component. Some traces of ...

2018年8月4日 · The $\mathrm{p}K_\mathrm{a}$ values for $\ce{H3AsO4}$ and $\ce{H3PO4}$ are $2.30$ and $2.12$ which indicate that $\ce{H3PO4}$ is a stronger acid compared to $\ce{H3AsO4}$.

2016年3月10日 · $$\ce{2H2SO4 <=> H3SO4+ + HSO4-}$$ Phosphoric acid is a weak acid and does not have such interactions and only loses protons (in equilibrium) in the presence of water. The autoprotolysis is important because through autoprotolysis, sulfuric acid now forms ion-ion interactions, which are much stronger interactions than hydrogen bonding.

2014年8月16日 · Sulfuric acid is such a strong acid, that it is capable of protonating any solvent that has a lone pair, even itself via autoprotolysis (in concentrated $98\%$ solution). $$\ce{2H2SO4 <=> [H3SO4]+ + [HSO4]- <=> H3+O + [HS2O7]- <=> H2O + H2S2O7}$$ The use of concentrated sulfuric in organic synthesis is usually not advisable, since its ...

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2013年8月3日 · $\ce{HSO4-}$ look at the valencies of the hydrogen and sulphate ion, because of the numbers don't match i.e. hydrogen has a +1 charge that means it is deficient by 1 electron while sulphate has a -2 charge which means it has two extra electrons (it can also be viewed that it wants to 'give away' these two electrons) these valence numbers basically show the amount of bonds the molecules can ...

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2018年6月17日 · Apologies for this extremely basic question, I'm just beginning with Chemistry so please don't be too harsh on me. My book says that sulfuric acid, $\\ce{H2SO4}$, dissociates in its ions following ...