Choose the case that is not a Bronsted conjugate acid-base...

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00:02 There, in this question we are working with conjugate acid -base pairs.

00:06 So we need to start off by defining what those are.

00:10 Conjugate acid -base pairs refer to two species, in other words two formulas, that differ by a single, that means just one, hydrogen ion.

00:34 The acid has it, the conjugate base does not.

00:38 All right, so let's start looking at our options here.

00:41 We're looking for the one that is not a conjugate acid -base pair using this definition.

00:47 So for the first one, we have hco3 negative and co3 with a 2 negative charge.

01:00 Well sure enough, these differ by one hydrogen.

01:03 The hco3 acid and the co3 2 negative does not have that h+.

01:09 Remember if we take away an h +, we have one less plus there.

01:13 So that's why it went from negative one to negative two.

01:16 So this one is okay.

01:18 It is a base or it is a conjugate acid -base pair.

01:21 So that's not our answer.

01:24 So number one is not our answer.

01:26 Let's look at the second one.

01:28 The second one we have the hydronium ion h3o plus and water.

01:36 Well sure enough, these differ by one hydrogen.

01:40 If we take one hydrogen away, we get h2o instead of h3o.

01:45 So that one's a conjugate acid -base pair.

01:48 Let's look at the third pair...

Choose the case that is not a Bronsted conjugate acid-base pair. 1) $H_3BO_3$, $H_2BO_3$ 2) $CH_3NH_3^+$, $CH_3NH_2$ 3) $HCIO_2$, $CIO_2^-$ 4) $HCO_2H$, $HCOH$ 5) $HCN$, $CN^-$