How would you complete and balance the acid base neutralizations reaction: #HBr + Ba(OH)_2 ->#?

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Answer 1 · 2017-03-27T02:58:42

#2"HBr" + "Ba(OH)"_2 -> "BaBr"_2 + 2 "H"_2"O"#

In a neutralization reaction, if the base is a hydroxide, then the products formed would be the salt and water.

acid + base #-># salt + water

The water (#"H"_2"O"#) is a result of the combination of the #"H"^+# from the acid and the #"OH"^-# from the base.

The salt (#"BaBr"_2#) is simply the remaining anion of the acid (#"Br"^-#) and the cation of the base (#"Ba"^{2+}#).

The unbalanced equation is therefore

#"HBr" + "Ba(OH)"_2 -> "BaBr"_2 + "H"_2"O"#

To balance the equation, first notice that the number of Ba on both sides are the same. Ba is balanced.

Next, notice that the LHS is short of 1 x Br. So balance it by adding 1 unit of HBr.

#"2HBr" + "Ba(OH)"_2 -> "BaBr"_2 + "H"_2"O"#

Now, the RHS is missing 2 x H and 1 x O. Balance that by adding 1 units of #"H"_2"O"#.

#"2HBr" + "Ba(OH)"_2 -> "BaBr"_2 + 2"H"_2"O"#

Now, all the elements have equal amounts on both sides of the equation. The chemical equation is now considered balanced.