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 $\ce{H2O}$?

  • 1
    $\begingroup$ "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
    Commented Aug 30, 2014 at 13:56

1 Answer 1


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:

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

  • $\begingroup$ But here it does \n't follow thw basic ideo of bronsted lowry base $\endgroup$
    – DSinghvi
    Commented Aug 30, 2014 at 15:31
  • 2
    $\begingroup$ It does if you envision it dissociating first, which it will do in aqueous media. $\endgroup$
    – user7232
    Commented Aug 30, 2014 at 22:56
  • $\begingroup$ @JannisAndreska, but then where does the H30 hydronium ion come from in your second equation? Where was it in the first place? $\endgroup$ Commented Apr 28 at 1:50

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service and acknowledge you have read our privacy policy.

Not the answer you're looking for? Browse other questions tagged or ask your own question.