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It is well known fact that Barium Hydroxide is a base. How does the Brønsted-Lowry concept explain $\ce{Ba(OH)2}$ as a base?

Is it that $\ce{Ba(OH)2}$ first accepts a proton then leaves behind $\ce{H2O}$?

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    $\begingroup$ "Is it that Ba(OH)2 first accepts a proton then leaves behind H2O?" You know that's a really interesting statement; if you want to explore mechanisms of acidity, try checking out this thread: chemistry.stackexchange.com/questions/14165/… $\endgroup$ – Dissenter Aug 30 '14 at 13:56
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Barium hydroxide – or more exactly, the hydroxide ion – is a Brønsted-Lowry base, because in aqueous solution, it is completely dissociated into $\ce{Ba^2+}$ and $\ce{OH-}$ ions:

$$\ce{Ba(OH)2 -> Ba^2+ + 2OH-}$$

$\ce{OH-}$ is a proton acceptor, forming $\ce{H2O}$. In aqueous solution, the following reaction takes place:

$$\ce{OH- + H3O+ ->~ 2H2O}$$

Barium hydroxide thus reacts with acids in a neutralization reaction, with water and the barium salt of the respective acid as the products. For example, with hydrochloric acid:

$$\ce{Ba(OH)2 + 2HCl ->~ BaCl2 + 2H2O}$$

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  • $\begingroup$ But here it does \n't follow thw basic ideo of bronsted lowry base $\endgroup$ – DSinghvi Aug 30 '14 at 15:31
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    $\begingroup$ It does if you envision it dissociating first, which it will do in aqueous media. $\endgroup$ – user7232 Aug 30 '14 at 22:56

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