Question

How would you complete and balance the acid base neutralizations reaction: \[{ HBr}+{ Ba}{{\left( {OH} \right)}_{{2}}}\]?

Answer 1

Hint: A chemical equation is the chemical formula that provides the information of the elements and molecules that are reacting as well as the molecules that are being produced from that reaction.

Complete step by step answer:
The Law of Conservation of Mass states that the mass of the reactants must balance the mass of the products. To balance a chemical equation, the atoms of both the elements and molecules on the reactant side (left side) and product side (right side) must be equal to each other.
The chemical equation is balanced, meaning that equal numbers of atoms for each element involved in the reaction are represented on the reactant and product sides. This is a requirement the equation must satisfy to be consistent with the law of conservation of matter.
If an element appears in more than one formula on a given side of the equation, the number of atoms represented in each must be computed and then added together.
In a neutralization reaction, if the base is a hydroxide, then the products formed would be the salt and water.
acid+base$\to$ salt+water
The water \[\left( {{{H}}_{{2}}}{O} \right)\] is a result of the combination of the \[{{{H}}^{+}}\] from the acid and the \[{O}{{{H}}^{-}}\] from the base.
The salt \[\left( {BaB}{{{r}}_{{2}}} \right)\] is simply the remaining anion of the acid \[\left( {B}{{{r}}^{-}} \right)\] and the cation of the base\[\left( {Ba}_{{2}}^{+} \right)\] .
The unbalanced equation is therefore
\[{HBr}+{Ba}{{\left( {OH} \right)}_{{2}}}\to {BaB}{{{r}}_{{2}}}+{{{H}}_{{2}}}{O}\]
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 $1\times {Br}$. So balance it by adding $1$ unit of \[{HBr}\] .
\[{2HBr}+{Ba}{{\left( {OH} \right)}_{{2}}}\to {BaB}{{{r}}_{{2}}}+{{{H}}_{{2}}}{O}\]
Now, the RHS is missing \[2\times{H\; and\; }1{ }\times{O}.\]
Balance that by adding $1$ unit of \[{{{H}}_{{2}}}{O}\] . \[{2HBr}+{Ba}{{\left( {OH} \right)}_{{2}}}\to {BaB}{{{r}}_{2}}+{2}{{{H}}_{{2}}}{O}\]

Note: It may be confirmed by simply summing the numbers of atoms on either side of the arrow and comparing these sums to ensure they are equal. Note that the number of atoms for a given element is calculated by multiplying the coefficient of any formula containing that element by the element’s subscript in the formula
Now, all the elements have equal amounts on both sides of the equation then only the chemical equation is now considered balanced.