why hydrogen ions can't exist alone???
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Answered by
19
H+ cannot exist in free state practically cause, in a solution in which water or any polar solvent is used, the H+ ion is hydrolyzed to form H3O+ ion, hydration energy is higher for H3O+ so it's more stable, also protonation of ions results in formation of more stable bronsted Lowry acid bases. Also zundel cation H502+, eigen cation H9O4+ play an important role in proton diffusion
The above case of H+ is just due to the self ionization of water, there are many examples which show this phenomenon based on bronsted Lowry acid bases theory of strong and weak acids, solvation and hydration energies and also equilibrium constants play role in their formation
Water has very low ionization constant so it's possible that other polar solvents with low ionization constants show this behavior
The above case of H+ is just due to the self ionization of water, there are many examples which show this phenomenon based on bronsted Lowry acid bases theory of strong and weak acids, solvation and hydration energies and also equilibrium constants play role in their formation
Water has very low ionization constant so it's possible that other polar solvents with low ionization constants show this behavior
Answered by
30
Because the bare nucleus can readily combine with other particles (electrons, atoms, and molecules), the isolated hydrogen ion can exist only in a nearly particle-free space (high vacuum) and in the gaseous state.
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