Write complete ionic and net ionic equations for each of the...

Write complete ionic and net ionic equations for each of the following reactions. $$\begin{array}{l}{\text { a. } \mathrm{K}_{2} \mathrm{S}(\mathrm{aq})+\mathrm{CoCl}_{2}(\mathrm{aq}) \rightarrow 2 \mathrm{KCl}(\mathrm{aq})+\mathrm{CoS}(\mathrm{s})} \\ {\text { b. } \mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{CaCO}_{3}(\mathrm{s}) \rightarrow} \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{CO}_{2}(\mathrm{g})+\mathrm{CaSO}_{4}(\mathrm{s})\\ {\text { c. } 2 \mathrm{HClO}(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq}) \rightarrow} \\ {2 \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{Ca}(\mathrm{ClO})_{2}(\mathrm{aq})}\end{array}$$

Write complete ionic and net ionic equations for each of
the following reactions.
$$\begin{array}{l}{\text { a. } \mathrm{K}_{2} \mathrm{S}(\mathrm{aq})+\mathrm{CoCl}_{2}(\mathrm{aq}) \rightarrow 2 \mathrm{KCl}(\mathrm{aq})+\mathrm{CoS}(\mathrm{s})} \\ {\text { b. } \mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{CaCO}_{3}(\mathrm{s}) \rightarrow} \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{CO}_{2}(\mathrm{g})+\mathrm{CaSO}_{4}(\mathrm{s})\\ {\text { c. } 2 \mathrm{HClO}(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq}) \rightarrow} \\ {2 \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{Ca}(\mathrm{ClO})_{2}(\mathrm{aq})}\end{array}$$

Key Concepts

Solubility Rules

Solubility rules are guidelines used to predict whether an ionic compound will dissolve in water. These rules help determine whether compounds will appear as dissociated ions in solution or as precipitates in complete and net ionic equations, thereby influencing how reactions are represented.

Spectator Ions

Spectator ions are ions present in the reaction mixture that remain unchanged on the reactant and product sides of the equation. They do not participate in the formation of the precipitate, gas, or weak electrolyte and are omitted from the net ionic equation to simplify the representation of the actual chemical change.

Precipitation Reactions

Precipitation reactions occur when two aqueous solutions combine to form an insoluble solid, known as a precipitate. Recognizing a precipitation reaction is crucial in writing ionic equations since the precipitate is represented in its undissociated form, while the soluble ions are depicted as individual species.

Complete Ionic Equation

A complete ionic equation breaks down all strong electrolytes into their constituent ions in aqueous solution while representing precipitates, gases, or weak electrolytes in their intact form. It shows every ion present in the reaction and provides a detailed picture of the species that exist in solution.

Net Ionic Equation

The net ionic equation filters out the spectator ions—those ions which do not participate in the chemical change—to show only the species that actually undergo a chemical transformation. It represents the essence of the reaction by focusing solely on the reactants and products that change during the process.

Transcript

00:01 Okay, now we do problem 99.

00:03 So we have to write ionic equation and the not ionic equation for this kind of problem.

00:09 You have to keep in mind with electrolytes, solid and gas, we don't separate.

00:17 We don't separate iron.

00:19 We don't separate this kind of compound into carty and an ion when we write in the arn equation.

00:29 Ionet equation, sorry.

00:32 So problem question a, we have potassium sulfide and couple 2 chloride.

00:40 And they reduce potassium chloride and couple sulfide.

00:44 And then we see only couple sulfide show that the rest are accurate so we can separate them.

00:51 And before you separate them, you have to see if the equation balance or not.

00:57 You have to balance them before you write ionic equation.

00:59 And then you see on the ball, i separate them.

01:04 And after i separate them, i look at both sides.

01:07 So which iron both sides also have? so i have to submit them, admit them.

01:14 This iron will call spectator iron.

01:18 Okay? so i submit potassium chloride.

01:24 So i have only the left side, cobal two iron and sulfide.

01:29 Left so i write them.

01:31 And the left side i have a couple sulfide.

01:33 I keep this i don't separate because they're solid.

01:37 For the next question, the b, we know calcium force calcium carbonate is solid.

01:47 Calcosylsulfate in this equation, they show solid.

01:50 They dissolve very little, so consider insoluble.

01:54 So good water and gas, right? so only are, you.

02:00 I see, is accurate so we can separate these compounds into potassium, antoca and anion...

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