Rewrite the following balanced equations as net ionic...

Rewrite the following balanced equations as net ionic equations. (a) $\mathrm{Na}_2 \mathrm{SO}_4(a q)+\mathrm{BaCl}_2(a q) \longrightarrow \mathrm{BaSO}_4(s)+2 \mathrm{NaCl}(a q)$ (b) $6 \mathrm{NaOH}(a q)+3 \mathrm{Cl}_2(\mathrm{~g}) \longrightarrow$ $$ \mathrm{NaClO}_3(a q)+5 \mathrm{NaCl}(a q)+3 \mathrm{H}_2 \mathrm{O}(\ell) $$ (c) $\mathrm{Hg}_2\left(\mathrm{NO}_3\right)_2(a q)+2 \mathrm{Kl}(a q) \longrightarrow \mathrm{Hg}_2 \mathrm{I}_2(s)+2 \mathrm{KNO}_3(a q)$ (d) $3 \mathrm{NaOCl}(a q)+\mathrm{KI}(a q) \longrightarrow$ $$ \mathrm{NaIO}_3(a q)+2 \mathrm{NaCl}(a q)+\mathrm{KCl}(a q) $$

Rewrite the following balanced equations as net ionic equations.
(a) $\mathrm{Na}_2 \mathrm{SO}_4(a q)+\mathrm{BaCl}_2(a q) \longrightarrow \mathrm{BaSO}_4(s)+2 \mathrm{NaCl}(a q)$
(b) $6 \mathrm{NaOH}(a q)+3 \mathrm{Cl}_2(\mathrm{~g}) \longrightarrow$
$$
\mathrm{NaClO}_3(a q)+5 \mathrm{NaCl}(a q)+3 \mathrm{H}_2 \mathrm{O}(\ell)
$$
(c) $\mathrm{Hg}_2\left(\mathrm{NO}_3\right)_2(a q)+2 \mathrm{Kl}(a q) \longrightarrow \mathrm{Hg}_2 \mathrm{I}_2(s)+2 \mathrm{KNO}_3(a q)$
(d) $3 \mathrm{NaOCl}(a q)+\mathrm{KI}(a q) \longrightarrow$
$$
\mathrm{NaIO}_3(a q)+2 \mathrm{NaCl}(a q)+\mathrm{KCl}(a q)
$$

Key Concepts

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the number of each type of atom and the overall charge are conserved on both sides of the reaction. This principle, based on the law of conservation of mass and charge, is essential for accurately describing any chemical reaction.

Complete Ionic Equations

Complete ionic equations represent all the soluble ionic compounds as their respective ions in aqueous solution. This detailed depiction is the starting point for deriving net ionic equations by allowing the identification and removal of spectator ions.

Solubility Rules

Solubility rules are guidelines that help predict whether an ionic compound will dissolve in water or form a precipitate. When writing net ionic equations, these rules are crucial for determining which compounds exist as ions in solution and which form the insoluble products that precipitate out of the reaction.

Net Ionic Equations

Net ionic equations are simplified chemical equations that only include the species that participate directly in the chemical change. By eliminating the spectator ions, these equations provide a focused view of the actual chemical reaction process, highlighting the fundamental interactions between the reacting species.

Spectator Ions

Spectator ions are ions present in the reaction mixture that do not undergo any chemical change during the course of the reaction. They appear unchanged on both sides of the complete ionic equation and can be omitted when writing the net ionic equation, as they do not affect the overall reaction mechanism.

Transcript

00:01 In this question we've been given some chemical reactions and we've been asked to balance them out and then write the net ionic equation.

00:08 So for the first one, the balanced chemical reaction of the system that we have been given, this is going to be two moles of silver nitrate reacting with sodium sulphide to form silver sulphide plus two moles of sodium nitrate.

00:25 So once we have this chemical reaction that is balanced, we then need to write the net ionic acid.

00:30 Equation and for us to write the net ionic equation we first of all have to determine the species that actually form ions in solution and those are going to be the ones that have an acrier state so all of these are going to be having an acar state except for our silver sulphite which is the solid or precipitate now that we have identified these we just need to look into which ions are being formed by these species that are in aqueer solution looking at silver nitrite we're going to be forming two moles of silver ions plus two more of nitrate ions.

01:04 And then for the silver, for the sodium sulfide, we're going to be forming two more of sodium ions plus a more of sulfide ions and we're going to be forming two more of sodium ions plus two more of nitrate ions from this sodium nitrate.

01:23 And finally our precipitate, which is silver sulfide.

01:27 So to write the net ionic equation, we need to remove the spectator.

01:31 Specter ions and these are the nitrate ions and the sodium ions.

01:36 Spectrater ions are those that are common in the reactants and the products.

01:41 So what is actually happening here is we have our sulphite ions in archaeus solution reacting with two moles of silver ions in arquia solution to form a hes solid precipitate.

01:55 And then moving on to the next one, this is just the approach that we are going to be using.

01:59 That is, we first of all write a balanced chemical equation.

02:03 Look at the species that actually form ions in solution.

02:06 Form those ions, remove the spectator ions and write out the net ionic equation...

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