Complete and balance each of the following neutralization...

Complete and balance each of the following neutralization reactions, name the products, and write the net ionic equations. a. $\mathrm{HI}(a q)+\mathrm{LiOH}(a q) \rightarrow$ b. $\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{KOH}(a q) \rightarrow$ c. $\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{CH}_{3} \mathrm{COOH}(a q) \rightarrow$ d. $\mathrm{HNO}_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightarrow$

Complete and balance each of the following neutralization reactions, name the products, and write the net ionic equations.
a. $\mathrm{HI}(a q)+\mathrm{LiOH}(a q) \rightarrow$
b. $\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{KOH}(a q) \rightarrow$
c. $\mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{CH}_{3} \mathrm{COOH}(a q) \rightarrow$
d. $\mathrm{HNO}_{3}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightarrow$

Key Concepts

Acid and Base Strength

The strength of an acid or a base refers to its propensity to ionize in solution. Strong acids and bases ionize completely, providing a straightforward representation in ionic equations, while weak acids and bases only partially ionize, which can influence the way the reaction is depicted in both complete and net ionic equations.

Spectator Ions

Spectator ions are ions present in the reaction mixture that do not participate in the actual chemical change. They appear unchanged on both the reactant and product sides of the complete ionic equation and are omitted in the net ionic equation to focus on the reactive species.

Net Ionic Equations

Net ionic equations simplify the reaction by removing spectator ions—ions that do not participate in the chemical change—in order to highlight only the species that actually change during the reaction. This provides a clearer picture of the fundamental chemical process occurring in the reaction.

Balancing Chemical Equations

Balancing chemical equations involves adjusting the coefficients of reactants and products to ensure that the number of each type of atom is conserved on both sides of the equation. This process adheres to the law of conservation of mass, ensuring that matter is neither created nor destroyed in a chemical reaction.

Neutralization Reactions

Neutralization reactions are chemical reactions in which an acid and a base react to form water and a salt. In these reactions, the hydrogen ions (H?) from the acid combine with the hydroxide ions (OH?) from the base to produce water, while the remaining ions form various salts.

Complete Ionic Equations

A complete ionic equation breaks down all soluble strong electrolytes into their constituent ions. This approach provides a detailed view of all the species present in the solution, which is essential for understanding and analyzing the actual chemical processes taking place during a reaction.

Transcript

00:01 This question combines your understanding of chemical equations with acid -based reactions, solubility rules, and netionic equations.

00:16 So the first reaction is h .i.

00:20 Aqueous with lithium hydroxide.

00:22 Hopefully you recognize this as an acid and a base, and the h .i.

00:29 Is going to donate a hydrogen to lithium -hydroxide, creating lithium iodide and water.

00:39 From solubility rules and recognizing this is a strong acid and this is a strong base, a strong acid will completely dissociate into its ions, as will the strong base.

00:51 Lithium iodide, according to solubility rules, also dissociates into its ions, lithium and iodide, where water stays as a liquid.

01:01 So, if we cancel the spectator ions, we see that the lithiums will cancel, the iodides will cancel, and the netionic equation will become hydrogen ion plus hydroxide produces water.

01:18 For the next one, we have phosphoric acid reacting with potassium hydroxide.

01:24 According to solubility rules and recognizing our strong acids and strong bases, this is a strong base that will completely dissociate.

01:35 This is not one of the strong acids that you would have memorized so it does not dissociate.

01:41 However the reaction will still occur while where these hydrogens will be donated to the hydroxides coming from multiple potassium hydroxides in order to generate potassium phosphate which according to solubility rules is aqueous.

01:58 We then need to balance it recognizing to get the three potassiums here, we need three potassium hydroxides, which gives us three waters.

02:10 Then we write the ionic equation.

02:13 Phosphoric acid does not separate.

02:16 Potassium hydroxide does.

02:18 Potassium phosphate does, and water stays as a liquid...

Please give Ace some feedback