Answered

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14. Which net ionic equation describes the reaction between K3PO4( aq) when it is mixed
with Al(NO3)3( aq)?

Al 3+( aq) + PO43-( aq) - AlPO4( s)
-
K+(aq) + NO3(aq) - KNO3(aq)
Al 3+( aq) +3NO3 -(aq) - 3AINO3( s)
-
3K +(aq) + PO43-( aq) – 3KPO4( s)

Sagot :

Explanation:

The net ionic equation is a chemical equation that depicts the elements, molecules, or ions that are directly involved in the chemical reaction itself. Likewise, spectator ions which is an ion that does not take part in the chemical equation where such species would be found in the solution both before and after the reaction.

Net ionic equations, similar to molecular equations, must be balanced not only by mass but also by charge. This implies that the overall charge of the net ionic equation is zero, or neutral. Lastly, only molecules in aqueous state can be separated into their ionic form.

Considering the reaction between potassium phosphate, [tex]K_{3}PO_{4}[/tex], and aluminium nitrate, [tex]Al(NO)_{3}[/tex]. The balanced molecular equation of the reaction is

         [tex]K_{3}PO_{4} \ (aq) \ + \ Al(NO_{3})_{3} \ (aq) \quad \longrightarrow \quad 3KNO_{3} \ (aq) \ + \ AlPO_{4} \ (s)[/tex].

*Note that aluminium phosphate is in a solid state (precipitation) because it is an insoluble salt whereas potassium nitrate is a soluble salt.

Separate the molecules in the aqueous state into their ionic components.

   [tex]3K^{+} \ (aq) \ + \ {PO_{4}}^{3-} \ (aq) \ + \ Al^{3+} \ (aq) \ + \ 3NO_{3} \ (aq) \quad \longrightarrow \quad 3K^{+} \ (aq) \ +[/tex]

                                                                                                        [tex]\ 3NO_{3} \ (aq) \ +[/tex]

                                                                                                          [tex]AlPO_{4} \ (s)[/tex]

Canceling out the spectator ions yields the net ionic equation for the reaction.

                               [tex]Al^{3+} \ (aq) \ + \ {PO_{4}}^{3-} \ (aq) \quad \longrightarrow \quad AlPO_{4} \ (s)[/tex]

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