Question

How do you balance ${\text{Ni}}{\left( {{\text{N}}{{\text{O}}_{\text{3}}}} \right)_{\text{2}}} + {\text{NaOH}} \to {\text{Ni}}{\left( {{\text{OH}}} \right)_{\text{2}}} + {\text{NaN}}{{\text{O}}_{\text{3}}}$?

Answer 1

Hint:To balance the given reaction we must know that in a balanced chemical equation the number of all the atoms of the elements present in the chemical reaction are equal. A symbolic representation of a chemical reaction which has an equal number of atoms of each element in the product and the reactant is known as a balanced chemical equation.

Complete step by step solution:
We know that a symbolic representation of a chemical reaction which has an equal number of atoms of each element in the product and the reactant is known as a balanced chemical equation.
To balance the given reaction we must know that in a balanced chemical equation the number of all the atoms of the elements present in the chemical reaction are equal.
The given reaction is as follows:
${\text{Ni}}{\left( {{\text{N}}{{\text{O}}_{\text{3}}}} \right)_{\text{2}}} + {\text{NaOH}} \to {\text{Ni}}{\left( {{\text{OH}}} \right)_{\text{2}}} + {\text{NaN}}{{\text{O}}_{\text{3}}}$
In the given reaction, we can consider the nitrate ion i.e. ${\text{NO}}_3^ - $ ion and the hydroxide ion i.e. ${\text{O}}{{\text{H}}^ - }$ ion an a whole entity rather than separately calculating each atom in the ions.
In the given reaction, there are 2 nitrate ions on the reactant side and only 1 nitrate ion on the product side.
Thus, to balance the number of nitrate ions change the coefficient of the product i.e. ${\text{NaN}}{{\text{O}}_{\text{3}}}$ to 2. Thus, the reaction is as follows:
${\text{Ni}}{\left( {{\text{N}}{{\text{O}}_{\text{3}}}} \right)_{\text{2}}} + {\text{NaOH}} \to {\text{Ni}}{\left( {{\text{OH}}} \right)_{\text{2}}} + 2{\text{NaN}}{{\text{O}}_{\text{3}}}$
Now, there are 2 sodium atoms on the product side and 1 sodium atom on the reactant side.
Thus, to balance the number of sodium atoms change the coefficient of the reactant i.e. ${\text{NaOH}}$ to 2. Thus, the reaction is as follows:
${\text{Ni}}{\left( {{\text{N}}{{\text{O}}_{\text{3}}}} \right)_{\text{2}}} + 2{\text{NaOH}} \to {\text{Ni}}{\left( {{\text{OH}}} \right)_{\text{2}}} + 2{\text{NaN}}{{\text{O}}_{\text{3}}}$
Thus, the balanced chemical equation is as follows:
${\text{Ni}}{\left( {{\text{N}}{{\text{O}}_{\text{3}}}} \right)_{\text{2}}} + 2{\text{NaOH}} \to {\text{Ni}}{\left( {{\text{OH}}} \right)_{\text{2}}} + 2{\text{NaN}}{{\text{O}}_{\text{3}}}$

Note: Remember that to balance any chemical equation first count each atom on the reactant and product side. Then balance each atom by changing the co-efficients. Balanced chemical equations are important in determining the stoichiometry of the reaction.