What is the conjugate base of each of the following acids?...

What is the conjugate base of each of the following acids?
(a) $\mathrm{NH}_{3}$
(b) $\mathrm{H}_{2} \mathrm{O}$
(c) $\mathrm{H}_{2}$
(d) $\mathrm{HC}=\mathrm{CH}$
(e) $\mathrm{CH}_{3} \mathrm{OH}$
(f) $\mathrm{H}_{3} \mathrm{O}^{+}$

Key Concepts

Bronsted-Lowry Acid-Base Theory

The Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. This concept is fundamental in understanding acid-base reactions, including the formation of conjugate bases when acids release a proton.

Deprotonation Process

Deprotonation is the process by which a molecule loses a proton. This process transforms an acid into its conjugate base, highlighting the dynamic equilibrium between protonated and deprotonated forms in acid-base chemistry.

Conjugate Base

A conjugate base is the species that remains after an acid has donated a proton (H+). In acid-base reactions, every acid has a corresponding conjugate base, which is its ionized form that can potentially accept a proton back, thereby reversing the reaction.

Transcript

00:01 All right, so for problem 20, we have to find the conjugate base for all these acids.

00:05 And it's really not that hard.

00:07 All you do is pretend that these acids reacted with some other base.

00:11 And when they do that, they donate a proton or an h plus ion.

00:16 So what you do is you simply like subtract a hydrogen from like the number of hydrogens it has.

00:24 And you subtract the one from the net charge or the total charge.

00:29 Since you're donating a proton, you're like subtracting a positively charged particle from it, which means that the conjugate base will usually be like more negatively charged.

00:43 But basically, this is what we're going to do.

00:45 So for a, we have ammonia.

00:48 So it's going to donate a proton, so we subtract one of the hydrogens.

00:53 So it's going to be nh2.

00:56 But since we donate a proton, which is a positively charged, charged the particle.

01:01 This has a negative overall charge since now the electrons outnumber the protons in this conjugate base because we donated a proton.

01:17 And for b we have water.

01:20 So all we do is just to remove one of the hydrogen.

01:23 So we're just going to have oxygen and one and it's going to be negatively charged, like i said before, and this will just be a hydroxide ion.

01:35 And we just do the same for the rest, so for c, we have a hydrogen molecule...

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