Respuesta :

jacob193

Answer:

Net ionic equation:

[tex]\rm Ag^{+}\; (aq) + Cl^{-}\; (aq) \to AgCl\; (s)[/tex].

Explanation:

Start by balancing the chemical equation. The acetate (IUPAC: ethanoate) ion [tex]\rm {C_2H_3O_2}^{-}[/tex] is a polyatomic ion. These ions stayed intact during this reaction. These ions could thus be considered as a monatomic ion [tex]\rm Ac^{-}[/tex] to make this equation easier to balance.

[tex]\rm ?\; AgAc\; (aq) + ?\; NiCl_2\;(aq)\to ?\; AgCl\; (s) + ?\;NiAc_2\; (aq)[/tex]

Assign a coefficient of 1 to [tex]\rm Ni(C_2 H_3O_2)[/tex]:

[tex]\rm ?\; AgAc\; (aq) + ?\; NiCl_2\;(aq)\to ?\; AgCl\; (s) + {\bf 1}\;NiAc_2\; (aq)[/tex]

[tex]\rm {\bf 2}\; AgAc\; (aq) + {\bf 1}\; NiCl_2\;(aq)\to ?\; AgCl\; (s) + 1\;NiAc_2\; (aq)[/tex]

[tex]\rm {2}\; AgAc\; (aq) + {1}\; NiCl_2\;(aq)\to {\bf 2}\; AgCl\; (s) + 1\;NiAc_2\; (aq)[/tex]

Rewrite this chemical equation as an ionic equation. For each salt in this reaction: if the salt dissolves in water, rewrite it as the ions that in produce. Don't rewrite species that won't dissolve into ions.

For example:

  • The salt [tex]\rm NiCl_2[/tex] is soluble in water. It dissolves to produce [tex]\rm Ni^{2+}[/tex] ions and [tex]\rm Cl^{-}[/tex] ions. Hence rewrite [tex]NiCl_2[/tex] as [tex]\rm Ni^{2+} + Cl^{-}[/tex]
  • The salt [tex]\rm AgCl\; (s)[/tex] is insoluble in water. Do not rewrite.

[tex]\begin{aligned}&\rm {2}\; Ag^{+} + 2\; Ac^{-}\; (aq) + Ni^{2+} + 2\;Cl^{-}\;(aq)\\\to &\rm {2}\; AgCl\; (s) + Ni^{+}\;(aq) + 2\; Ac^{-}\; (aq)\end{aligned}[/tex].

Eliminate terms that appear on both side of this equation.

[tex]\rm {2}\; Ag^{+} + 2\;Cl^{-}\;(aq) \to {2}\; AgCl\; (s)[/tex].

Simplify the coefficients:

[tex]\rm Ag^{+} + Cl^{-}\;(aq) \to AgCl\; (s)[/tex].

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