Decide which compound is the acid and which is the base, and draw the products of each proton tr

step 1 Okay, so today we're going to be going over question number five. And let's have CL CL CL here.

Decide which compound is the acid and which is the base, and...

Key Concepts

Conjugate Acid-Base Pairs

When a proton transfer reaction occurs, the reactant that donates a proton becomes a conjugate base, and the one that accepts the proton becomes a conjugate acid. These pairs are linked by the loss and gain of a proton and are central to the reversibility and equilibrium aspects of acid-base chemistry. Recognizing these pairs helps clarify reaction mechanisms and predict the direction of the equilibrium.

Proton Transfer Reaction

This type of reaction involves the movement of a proton from one species to another. Proton transfer reactions are the hallmark of acid-base interactions under the Brønsted–Lowry definition. Understanding these reactions is crucial since they form the basis for many biochemical and industrial processes, and they help illustrate the concept of dynamic equilibrium in solution.

Brønsted–Lowry Acid

This concept defines an acid as a substance that donates a proton (H+) during a reaction. In acid-base chemistry, identifying which compound is responsible for supplying the proton is key, as it determines the direction of the equilibrium and influences the overall reactivity. The focus is on the movement of the proton rather than electron pair exchange.

Brønsted–Lowry Base

A Brønsted–Lowry base is defined as a substance that accepts a proton during a reaction. Recognizing the base involves identifying the species capable of capturing a proton, which often leads to the formation of its conjugate acid. This identification is central to classifying the roles of reactants in proton transfer reactions.

Transcript

00:01 Okay, so today we're going to be going over question number five.

00:05 And let's have cl cl cl here.

00:18 Double one to two and o single one to two and oh plus och3.

00:30 You have your pairs of electrons.

00:34 And there is a minus charge.

00:36 So in this case, too, in order to identify which one of these is the acid and which one is the base, you have to look to see which one has the capability of donating a proton, and that will be your acid, and which one has the capability of accepting a proton, and that one will be your base.

00:59 So in this case, when you look at both of the two species, the one that can donate is going to, going to be your first one because you have your oh group.

01:14 So this is going to be your acid, which means this is going to be your base.

01:22 So your products since this species gave up its proton, it except this one will accept it.

01:38 So it's going to be ch3oh plus.

01:48 So you have, let's see, c l, carbon, cl, cl, carbon, double pointed to an o.

02:08 And then since it lost the hydrogen, you're going to have a hydrogen here.

02:14 But it's going to have a minus charge.

02:22 B, you have cl, cl.

02:27 Cl cl, cl.

02:33 And this one is triple bonded to an h plus h with its two electrons and a minus charge.

02:44 So on this case, the one that can't donate is going to be your first one.

02:49 So that is going to be your acid.

02:51 The second one is going to be your piece...

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