Question

Complete and balance the equation for the following acid-base neutralization reaction. If water is used as a solvent, write the reactants and products as aqueous ions. In some cases, there may be more than one correct answer, depending on the amount of reactants used.

(a)Mg(OH)2 + HClO4?
(b)SO3 + H2O? (Assume an excess of water and that the product dissolves)
(c) SrO + H2SO4?

Answer 1

Step-by-step explanation:

A balanced equation is defined as the one that has equal number of atoms of all the elements present on both reactant and product side.

(a)
`Mg(OH)_(2) + HClO_(4) \rightarrow Mg(ClO_(4))_(2) + H_(2)O`

Number of atoms on reactant side are as follows.

Mg = 1

O = 6

H = 3

Cl = 1

Number of atoms on product side are as follows.

Mg = 1

O = 9

H = 2

Cl = 2

So, to balance this equation we multiply
`Mg(OH)_(2)` by 2 on reactant side and multiply
`H_(2)O` by 2 on product side.

Therefore, the balanced reaction equation is as follows.

`2Mg(OH)_(2) + HClO_(4) \rightarrow Mg(ClO_(4))_(2) + 2H_(2)O`

(b)
`SO_(3) + H_(2)O \rightarrow H_(2)SO_(4)`

Number of atoms on reactant side are as follows.

S = 1

O = 4

H = 2

Number of atoms on product side are as follows.

S = 1

O = 4

H = 2

Therefore, this equation is balanced as it has same number of atoms on both reactant and product side.

(c)
`SrO + H_(2)SO_(4) \rightarrow SrSO_(4) + H_(2)O`

Number of atoms on reactant side are as follows.

Sr = 1

O = 1

H = 2

S = 1

O = 4

Number of atoms on product side are as follows.

Sr = 1

O = 1

H = 2

S = 1

O = 4

Therefore, this equation is balanced.