the is well known reality that Barium Hydroxide is a base. Just how does the Brønsted-Lowry principle explain $ceBa(OH)2$ together a base?

Is it that $ceBa(OH)2$ very first accepts a proton then pipeline behind $ceH2O$?



Barium hydroxide – or an ext exactly, the hydroxide ion – is a Brønsted-Lowry base, due to the fact that in aqueous solution, the is completely dissociated into $ceBa^2+$ and $ceOH-$ ions:

$$ceBa(OH)2 -> Ba^2+ + 2OH-$$

$ceOH-$ is a proton acceptor, creating $ceH2O$. In aqueous solution, the adhering to reaction takes place:

$$ceOH- + H3O+ ->~ 2H2O$$

Barium hydroxide for this reason reacts with acids in a neutralization reaction, through water and the barium salt that the particular acid together the products. For example, through hydrochloric acid:

$$ceBa(OH)2 + 2HCl ->~ BaCl2 + 2H2O$$

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edited Oct 29 "16 in ~ 16:59
reply Aug 30 "14 in ~ 13:15

Jannis AndreskaJannis Andreska
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$egingroup$ the does if friend envision the dissociating first, which it will execute in aqueous media. $endgroup$
Aug 30 "14 at 22:56
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