when solutions of silver perchlorate, a g c l o 4 ( a q ) agclox4(aq) , and ammonium iodide, n h 4 i ( a q ) nhx4i(aq) , are mixed, a solid precipitate forms, indicating a reaction. which species should appear in the net ionic equation representing the reaction? select one or more:

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25-10-2022
Chemistry

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when solutions of silver perchlorate, a g c l o 4 ( a q ) agclox4(aq) , and ammonium iodide, n h 4 i ( a q ) nhx4i(aq) , are mixed, a solid precipitate forms, indicating a reaction. which species should appear in the net ionic equation representing the reaction? select one or more:

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contexto38 contexto38 · Answer 1 · 2022-11-02T10:19:21-04:00

The net ionic equation showing the reaction should show [tex]I^{-}[/tex], AgI, and [tex]Ag^{+}[/tex] species.

A net ionic equation is defined as an equation that only represents the ions or molecules that are actively participating in the reaction or those that change. The spectator ions are absent from this equation.

A substance's solubility refers to its capacity to combine with another substance the solvent to produce a solution. The opposing property is called insolubility, which refers to the solute's inability to produce such a solution.

The products are AgI and [tex]NH_{4} CIO_{4}[/tex]

Iodide of [tex]Pb^{2+}[/tex], [tex]Ag^{+}[/tex] and [tex]Hg_{2} ^{2+}[/tex] are insoluble

So, AgI is not soluble

Ammonium Salts are soluble

So, [tex]NH_{4} CIO_{4}[/tex] is soluble

So, the reaction is:

[tex]AgClO_{4}[/tex](aq) + [tex]NH_{4} I[/tex](aq) ⇒ AgI(s) + [tex]NH_{4} CIO_{4}[/tex](aq)

Its net ionic equation would be:

[tex]Ag^{+}[/tex](aq) + [tex]I^{-}[/tex]aq) ⇒ AgI(s)

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