2 added 82 characters in body edited Oct 29 '16 at 16:59 Jannis Andreska 5,17911 gold badge3030 silver badges7676 bronze badges Barium hydroxide --– or more exactly, the hydroxide ion --– is a Brønsted-Lowry base, and thus itsbecause in aqueous solution, it is strongly alkaline.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: $$\ce{Ba(OH)2 + 2HCl ->~ BaCl2 + 2H2O}$$ Barium hydroxide -- or more exactly, the hydroxide ion -- is a Brønsted-Lowry base, and thus its aqueous solution is strongly alkaline. $$\ce{OH-}$$ 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: $$\ce{Ba(OH)2 + 2HCl ->~ BaCl2 + 2H2O}$$ 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: $$\ce{Ba(OH)2 + 2HCl ->~ BaCl2 + 2H2O}$$ 1 answered Aug 30 '14 at 13:15 Jannis Andreska 5,17911 gold badge3030 silver badges7676 bronze badges Barium hydroxide -- or more exactly, the hydroxide ion -- is a Brønsted-Lowry base, and thus its aqueous solution is strongly alkaline. $$\ce{OH-}$$ 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: $$\ce{Ba(OH)2 + 2HCl ->~ BaCl2 + 2H2O}$$