Complete and balance each of the following neutralization reactions, name the products, and writ

Complete and balance each of the following neutralization...

Key Concepts

Neutralization Reaction

A neutralization reaction is a specific type of acid-base reaction where an acid and a base react quantitatively to form water and a salt. This reaction is central to understanding how acids and bases counteract each other, leading to a solution that is more neutral in pH.

Spectator Ions

Spectator ions are ions present in the reaction mixture that do not participate in the actual chemical change. They remain unchanged on both sides of the complete ionic equation and are omitted in the net ionic equation to simplify the representation of the reaction mechanism.

Net Ionic Equations

Net ionic equations streamline the complete ionic equations by removing spectator ions, thus highlighting only the species that are directly involved in the chemical reaction. This approach is particularly useful in acid-base neutralizations to focus on the fundamental proton transfer process.

Acid-Base Reactions

Acid-base reactions involve the chemical interaction between an acid, which donates protons (H+), and a base, which accepts protons. These reactions typically result in the formation of water and a salt, showcasing the fundamental properties of acids and bases as defined in the Brønsted-Lowry theory.

Balanced Chemical Equations

Balanced chemical equations ensure that the quantity of each element is conserved during the reaction. In the context of neutralization reactions, balancing the equation is essential to correctly represent the stoichiometry between the acid and the base, ensuring that all atoms and charges are accounted for in the product formation.

Complete Ionic Equations

Complete ionic equations break down all soluble ionic compounds into their individual ions, providing a clear picture of the species present in the solution. In neutralization reactions, this format helps identify which ions participate in the reaction and which exist as free ions in the solution.

Transcript

00:01 For problem 458, we have four chemical reactions that we need to complete, the products are not given, balance them, and then name the products, and then write the overall ionic and also the net ionic equation.

00:15 So this one does take a little bit of time.

00:19 We will take the two reactants that are given to us, hbr and potassium hydroxide, and through a disproportionation, or, or sometimes, i'm sorry, not disproportionation, through a metathesis reaction or a double displacement reaction, the cations exchange places and we end up with potassium bromide and then water as a liquid.

00:49 The hydrobromic acid is a strong acid, so it will separate into the hydrogen ion and the bromate anion.

00:56 Just like potassium hydroxide is a strong base, will separate into the potassium ion and the hydroxide anion.

01:02 Because potassium bromide salt is soluble in water, it will also separate into potassium ion and bromide anion, and then we'll still have our water as a liquid.

01:15 So this would be the formula equation, this would be the net, i'm sorry, this would be the full ionic equation.

01:22 We then cancel the ions that are commentable sides, these being spectator ions, and we end up with hydrogen, just reacting with hydroxide, producing.

01:32 Water.

01:33 This would be the net ionic equation.

01:37 Then for part b, we have phosphoric acid.

01:40 Phosphoric acid reacts with barium hydroxide, and in the process makes barium phosphate and six waters.

01:53 You'll notice that we have phosphate with a three minus charge and barium with a two plus charge.

02:03 So when those two guys get together, we're going to have three bariums and two phosphates.

02:08 So that's why we need a three here for barium hydroxide.

02:11 So we get three bariums and a two here for the two phosphates.

02:17 The two products then, as mentioned, are barium phosphate and water.

02:23 Now the ionic equation comes by recognizing which of these reactants and products are soluble in solution.

02:33 Phosphoric acid is a weak acid, and weak acids we assume stay together to the most significant extent with only few ions forming.

02:43 Barium hydroxide at low concentrations can be considered a strong base, and so it will separate into the barium ion and three barium ions and six hydroxide anions.

02:59 This then goes to barium phosphate, where remembering the solubility rules, this is insoluble, so it stays together as a solid.

03:08 And then water, of course, is a liquid...

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