Respuesta :
Explanation:
Complete ionic equation : In complete ionic equation, all the substance that are strong electrolyte and present in an aqueous are represented in the form of ions.
Net ionic equation : In the net ionic equations, we are not include the spectator ions in the equations. Only the species which are present in aqueous state dissociate.
Spectator ions : The ions present on reactant and product side which do not participate in a reactions. The same ions present on both the sides.
(a)
The balanced molecular equation will be,
[tex]2HClO_4_{(aq)}+Na_2CO_3_{(aq)}\rightarrow H_2O_{(l)}+CO_2_{(g)}+2NaClO_4_{(aq)}[/tex]
The complete ionic equation in separated aqueous solution will be,
[tex]2H^+_{(aq)}+2ClO_4^-_{(aq)}+2Na^+_{(aq)}+CO_3^{2-}_{(aq)}\rightarrow H_2O_{(l)}+CO_2_{(g)}+2Na^+_{(aq)}+2ClO_4^{-}_{(aq)}[/tex]
In this equation the species present are, [tex]2Na^+\text{ and }2ClO_4^-[/tex] are the spectator ions.
Hence, the net ionic equation contains specie is
[tex]2H^+_{(aq)}+CO_3^{2-}_{(aq)}\rightarrow H_2O_{(l)}+CO_2_{(g)}[/tex]
(b)
The balanced molecular equation will be,
[tex]NH_4Cl_{(aq)}+NaOH_{(aq)}\rightarrow H_2O_{(l)}+NH_3_{(g)}+NaCl_{(aq)}[/tex]
The complete ionic equation in separated aqueous solution will be,
[tex]NH_4^+_{(aq)}+Cl^-_{(aq)}+Na^+_{(aq)}+OH^{-}_{(aq)}\rightarrow H_2O_{(l)}+NH_3_{(g)}+Na^+_{(aq)}+Cl^{-}_{(aq)}[/tex]
In this equation the species present are, [tex]Na^+\text{ and }Cl^-[/tex] are the spectator ions.
Hence, the net ionic equation contains specie is
[tex]NH_4^+_{(aq)}+OH^{-}_{(aq)}\rightarrow H_2O_{(l)}+NH_3_{(g)}[/tex]
