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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