Write balanced complete ionic and net ionic equations for...

Write balanced complete ionic and net ionic equations for each reaction. a. $\operatorname{HCl}(a q)+\operatorname{LiOH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\operatorname{liCl}(a q)$ b. $\operatorname{MgS}(a q)+\operatorname{CuCl}_{2}(a q) \longrightarrow \operatorname{Cus}(s)+\operatorname{MgCl}_{2}(a q)$ c. $\mathrm{NaOH}(a q)+\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)$ d. $\mathrm{Na}_{3} \mathrm{PO}_{4}(a q)+\mathrm{NiCl}_{2}(a q) \longrightarrow \mathrm{Ni}_{3}\left(\mathrm{PO}_{4}\right)_{2}(\mathrm{s})+\mathrm{NaCl}(a q)$

Write balanced complete ionic and net ionic equations for each reaction.
a. $\operatorname{HCl}(a q)+\operatorname{LiOH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\operatorname{liCl}(a q)$
b. $\operatorname{MgS}(a q)+\operatorname{CuCl}_{2}(a q) \longrightarrow \operatorname{Cus}(s)+\operatorname{MgCl}_{2}(a q)$
c. $\mathrm{NaOH}(a q)+\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)$
d. $\mathrm{Na}_{3} \mathrm{PO}_{4}(a q)+\mathrm{NiCl}_{2}(a q) \longrightarrow \mathrm{Ni}_{3}\left(\mathrm{PO}_{4}\right)_{2}(\mathrm{s})+\mathrm{NaCl}(a q)$

Key Concepts

Complete Ionic Equation

A complete ionic equation represents all the soluble ionic compounds in an aqueous reaction as their constituent ions. It includes every ion present in the solution, which helps in understanding the full scope of species involved during the reaction, regardless of whether they directly participate in the actual chemical change.

Net Ionic Equation

A net ionic equation is a simplified version of the complete ionic equation that removes the spectator ions - those ions that do not undergo any change during the reaction. This equation focuses only on the actual chemical transformation by showing the essential reacting species and products.

Spectator Ions

Spectator ions are ions present in the reactants and products that do not participate directly in the chemical reaction. They remain unchanged on both sides of the complete ionic equation. Identifying and eliminating these ions is key to deriving the net ionic equation.

Acid-Base Reactions

Acid-base reactions, often exemplified by the neutralization process between an acid and a base, involve proton transfer. In ionic equations, strong acids and bases dissociate completely in water to form ions, and their reactions typically produce water and a salt, with appropriate balancing to account for the ions involved.

Precipitation Reactions

Precipitation reactions occur when two aqueous solutions containing ionic compounds combine to form an insoluble product, known as a precipitate. Recognizing these reactions involves determining whether the product of the ion exchange is insoluble in water, which is critical for constructing both complete and net ionic equations.

Solubility Rules

Solubility rules are guidelines that predict the solubility of ionic compounds in water. They help determine which compounds will remain dissolved and which will form precipitates. This knowledge is essential for deciding how to represent species in a complete ionic equation and for identifying the spectator ions that can be omitted from the net ionic equation.

Transcript

00:01 In order to write balanced complete ionic and net ionic equations for each reaction, we must first have a balanced formula equation.

00:11 Although the chemical reactions are provided, some of them are not balanced.

00:15 So we need to be aware of that before we proceed to writing the ionic and then the net ionic equation.

00:25 Here's the first reaction.

00:28 Hcl with lithium hydroxide will produce water and lithium chloride.

00:32 It is balanced as is.

00:34 Now to write the complete ionic equation.

00:38 Anything that is aqueous that will separate completely into ions needs to be written as ions.

00:45 H .c .l is a strong acid, so it will separate into h plus and cl minus.

00:50 Lithium hydroxide is a strong base, so it will separate into lithium ions and hydroxide an ions.

00:57 Water is not an ionic compound.

00:59 It stays together as h2o liquid.

01:02 Lithium chloride, however, according to solubility, rules is soluble, so it separates into lithium ion and chloride an ion.

01:12 This second equation is the complete ionic equation.

01:19 Once we get rid of the spectator ions that are common to both sides, chloride and lithium, what is left is what we call the net ionic equation.

01:31 Then we have magnesium sulfide reacting with copper two chloride to produce copper 2 sulfide, that's a solid, and magnesium chloride.

01:45 As written, it is balanced, so now we can separate all of the ionic compounds that are soluble into their corresponding ions.

01:53 Magnesium sulfide gives us a magnesium 2 plus and a sulfide 2 minus.

01:59 Copper 2 chloride gives us 1 copper 2 plus and 2cl minuses.

02:05 Copper 2 sulfide, according to solubility rules, is insoluble, so it stays together as a precipitate as a solid, but magnesium chloride is soluble, so we get a magnesium 2 plus and 2cl minuses.

02:20 This is a complete ionic equation.

02:23 Once we cancel the spectator ions that are common to both sides, magnesium and the two chlorides, what is left is then the net ionic equation.

02:34 The next one is sodium hydroxide reacting with acetic acid to produce water and sodium acetate.

02:43 It is balanced as written, so we can now proceed to the complete ionic equation...

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