Write net ionic equations for the following reactions: (a)...

Key Concepts

Net Ionic Equations

Net ionic equations simplify chemical reactions by removing spectator ions, showing only the species that undergo a chemical change. They help in understanding the fundamental chemical process without extraneous details.

Weak Electrolytes

Weak electrolytes, such as weak acids like acetic acid, do not completely dissociate in solution. Their limited ionization must be taken into account when writing net ionic equations, as they are typically represented in their molecular form.

Spectator Ions

Spectator ions are ions that remain unchanged on both sides of a chemical equation. They are omitted from net ionic equations, allowing focus on the actual chemical transformations occurring during the reaction.

Acid-Base Neutralization Reactions

Acid-base neutralization reactions involve the reaction of an acid and a base to form water and a salt. In net ionic form, these reactions often simplify to the underlying process of proton transfer between hydrogen ions and hydroxide ions.

Redox Reactions in Metal-Acid Reactions

Metal-acid redox reactions involve a metal reacting with an acid, resulting in the oxidation of the metal and reduction of hydrogen ions to form hydrogen gas. These reactions emphasize the electron transfer processes that occur in redox reactions.

Transcript

00:02 Okay, for this problem, we are going to look at two different reactions and write the net ionics.

00:08 Excuse me.

00:10 For a first reaction, we have acetic acid, and acetic acid is a weak acid.

00:22 That'll come into play in a little bit here.

00:24 And it's reacting with a strong base, which is sr, strontium hydroxide.

00:33 My products are going to be strontium acetate, which is ch3, co2, two that'll be aqueous plus water acid base reaction so this is an acid base reaction we've got a weak acid and a strong base okay so let's take a look at this we're going to have to get our chemical equation balanced and i'm probably going to need two of these there we go so now our next order of business is we're going to have to write a balanced chemical, we're going to have to write on a complete ionic equation.

01:24 And i'm going to do that, remembering that this weak acid, let me switch colors, is going to dissociate so little that it's going to be insignificant.

01:36 We're not even going to pay attention to it dissociating.

01:40 But the strontium hydroxide is going to dissociate almost 100 % because it's as strong.

01:48 There's 2 .0 .h.

01:50 Minus.

01:51 Strong base.

01:54 Now my strontium acetate is also going to dissociate and i've got ch3 co2 minus plus water.

02:16 There's my complete ionic equation.

02:20 So i'm going to be able to see that my, i would like to do these in orange, my strontium should be probably my only ions here that i'm going to be losing.

02:36 So let me rewrite this equation without the spectators.

02:42 C .h.

02:43 2.

02:44 Here's my molecular acid.

02:52 I'm going to have a couple of hydroxides left on the reactant side.

02:58 There's my arrow.

02:59 Not a very nice arrow.

03:01 There is the acetate ion...