Write balanced (i) formula unit, (ii) total ionic, and (iii)...

Write balanced (i) formula unit, (ii) total ionic, and (iii) net ionic equations for the reactions that occur between the acid and the base. Assume that all reactions occur in water or in contact with water. (a) lithium hydroxide $+$ sulfuric acid (b) calcium hydroxide $+$ phosphoric acid (c) copper(II) hydroxide $+$ nitric acid

Write balanced (i) formula unit,
(ii) total ionic, and (iii) net ionic equations for the reactions that occur between the acid and the base. Assume that all reactions occur in water or in contact with water.
(a) lithium hydroxide $+$ sulfuric acid
(b) calcium hydroxide $+$ phosphoric acid
(c) copper(II) hydroxide $+$ nitric acid

Key Concepts

Acid-Base Neutralization

Acid-base neutralization is a type of chemical reaction where an acid and a base react to form water and a salt. These reactions typically involve the transfer of a proton (H+) from the acid to the hydroxide ion (OH?) from the base, resulting in the formation of water. They are fundamental in chemistry, especially in understanding reaction mechanisms, titrations, and pH control in various systems.

Balanced Chemical Equations

Balanced chemical equations represent the conservation of mass and atoms in a reaction. This concept ensures that the number of atoms for each element, as well as the total charge, is the same on both sides of the equation. This is crucial for accurate stoichiometry, calculations in reaction conditions, and understanding the proportions in which reactants combine to form products.

Ionic Equations

Ionic equations are used to depict reactions in aqueous solutions by expressing compounds in terms of their constituent ions. The total ionic equation shows all the ions present in the solution, distinguishing soluble salts, acids, and bases dissociated into ions, which helps in identifying the species involved in the reaction.

Net Ionic Equations

Net ionic equations simplify the representation of reactions by omitting spectator ions—those ions that do not participate in the chemical change. This equation highlights only the ions and molecules directly involved in the reaction, thereby providing a clearer picture of the actual chemical process and the species undergoing transformation.

Transcript

00:01 So now let's write out these reactions and then write the ionic equations.

00:08 So then we have lithium hydroxide reacting with sulfuric acid.

00:11 Lithium hydroxide is soluble.

00:18 So these will switch partners and we need to balance out the charge within the ion as well.

00:25 So we need to refer to our solubility rules to see what phase everything is in.

00:31 If it's in the aqueous phase, it will be separated.

00:35 Into its ions.

00:40 So this is soluble, according to our solubility rules.

00:45 All sulfates are soluble except when paired with certain ions.

00:49 This is not one of the ions.

00:52 So we also get water because this is just a neutralization reaction.

00:56 The other reaction, the other product is water.

01:00 So now let's balance everything.

01:02 So we put a two here, and then we're going to put a two in front of the water.

01:12 Now we're going to split everything in aqueous phase into its ions.

01:38 Okay, so then, now let's cancel out what is on both sides, and then we'll get the net ionic as the equation for the neutralization between or the formation of water.

01:58 So we have hydrogen ion and hydroxide ion, giving us water.

02:05 Put the next one, this is in the solid phase, and this one is aqueous.

02:27 Then calcium is a charge of positive 2, phosphate a charge of negative 3.

02:45 This one is also insoluble...

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