Question

(d) AgC2H302(aq) + Nicl2(aq) → AgCl(s) + Ni(C2H302)2(aq)
What’s the ionic equation?

Answer 1

Net ionic equation:

`\rm Ag^(+)\; (aq) + Cl^(-)\; (aq) \to AgCl\; (s)`.

Step-by-step explanation:

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

`\rm ?\; AgAc\; (aq) + ?\; NiCl_2\;(aq)\to ?\; AgCl\; (s) + ?\;NiAc_2\; (aq)`

Assign a coefficient of 1 to
`\rm Ni(C_2 H_3O_2)`:

`\rm ?\; AgAc\; (aq) + ?\; NiCl_2\;(aq)\to ?\; AgCl\; (s) + {\bf 1}\;NiAc_2\; (aq)`

`\rm {\bf 2}\; AgAc\; (aq) + {\bf 1}\; NiCl_2\;(aq)\to ?\; AgCl\; (s) + 1\;NiAc_2\; (aq)`

`\rm {2}\; AgAc\; (aq) + {1}\; NiCl_2\;(aq)\to {\bf 2}\; AgCl\; (s) + 1\;NiAc_2\; (aq)`

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

`\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}`.

Eliminate terms that appear on both side of this equation.

`\rm {2}\; Ag^(+) + 2\;Cl^(-)\;(aq) \to {2}\; AgCl\; (s)`.

Simplify the coefficients:

`\rm Ag^(+) + Cl^(-)\;(aq) \to AgCl\; (s)`.