Many hunting dogs enjoy standing nose-to-nose with a skunk whi...

Question

Many hunting dogs enjoy standing nose-to-nose with a skunk while barking furiously, oblivious to the skunk spray directed toward them. One moderately effective way of lessening the amount of odor is to wash the dog in a bath containing dilute hydrogen peroxide, sodium bicarbonate, and some mild dish detergent. Use chemical reactions to describe how this mixture helps to remove the skunk spray from the dog. The two major components of skunk oil are 3-methylbutane-1-thiol and but-2-ene-1-thiol.

Accepted Answer

Hey, everyone. And welcome back when hunting dogs stand nose to nose with a skunk while barking furiously. They are often not aware of the skunk spray directed toward them. One method to reduce the amount of the order is to use a bath that contains some mild dish detergents, dilute hydrogen peroxide and sodium bicarbonate to wash the dog. If skunk oil contains two thol derivatives shown below, explain how using this mixture can help to remove the skunk spray and the two derivatives that were given are 33, the meth beats in one tile in three methyl beats two in one tile. Now, in this case, it's really important for us to remember that hydrogen peroxide can oxidize files and let's see how that works. So essentially we're going to take one of the two derivatives and we're going to repeat the process for the next one. But for now, let's concentrate on the first one, which is 33, then methyl butane one tile. So we have drawn the structure of the given derivative and whenever it undergoes oxidation with hydrogen peroxide, we get the following. First of all, let's recall that in the first step of the oxidation process, we are oxidizing the thol into sulfonic acid and essentially to draw it, we can draw the parent chain to begin with. And now what we're going to do is just replace the hydrogen with the O H group. OK. So we're simply incorporating oxygen between sulfur and hydrogen. And this is how we get sulfonic acid, which can later on be oxidized into another asset right leg to the process. If we keep oxidizing it, then we will get sulfuric acid. So we're going to add one more oxygen. Let's do that. Now, we have S O H and in addition to that, we're going to incorporate sulfur double bonded to another oxygen. This is how we get sulfuric acid and then we can even oxidize it further into sulfonic acid. So let's simply show that we're going to use another equivalent of hydrogen peroxide and we are getting sulfonic acid, which essentially corresponds to, to you S O groups. Rights. We're going to add two double bonded oxygens to that sulfur and then we still have our O H group, right? So that's how we're sulfonic acid. Well done. So now why is this really helpful for us? Now, what we understand is that gen peroxide oxidizes the thy into corresponding assets, right? We have a mixture of those assets and they are less volatile if they are less volatile, that essentially means they do not produce that this thing smell anymore, right? So that's really good for us because we want to lower the order. So because they're less volatile, we successfully do that. Now, another thing is OK, we have converted the file into acids so that we do not experience that smell. But now we need to wash the dog, right? So essentially what we're going to do, just as the problem suggests, we're going to use sodium bicarbonate, which essentially has bicarbonate anion H C 03 minus. And that's a basic and iron. So let's take one of the acids. Let's suppose we take sulfuric acid because it has that acidic proton bicarbonate captures that acidic proton to produce the conjugate base of sulfonic acid. And we can essentially illustrate the structure. Now, if we remove the acidic hydrogen, we are going to get negatively charged oxygen. So that's the conjugate base of sulfuric acid. And now because we have obtained a salt, right, specifically, because we're using sodium bicarbonate, we can say that we may simply add it as an spectator here and to our resultant salt because we have produced a salt. We now understand that it is water soluble, right? Because it's ionic, we have an ionic charge. Previously, we had a molecule. Now we end up with an ionic structure which means that it's water soluble. And now we understand that it can be washed away using soap. That's it. That's the whole logic. Now, it doesn't really matter which file derivative we use the other one has a double bond and no metal group. So even if we remove the metal group and simply add a double bond, nothing really will change. We will still get the same asset products, right. So let's go ahead and do that so that we can clearly see how we get our products when we consider the other thyle derivative. Also for the sulfonic acid, we should have added that methyl group and another metal group at position number two. But now considering the other file that we are analyzing, we have simply added one metal group. OK. And for the final product that is water soluble, we are simply going to remove our metal group and add a double bond. So the scheme is exactly the same and we are going to label it and just review everything because the analysis was not really short. And we are ready to conclude that first of all, the two style derivatives can be oxidized in a similar manner using hydrogen peroxide into a mixture of sulfuric acid, Sulfonic acid and sulfonic acid. The three acids are less volatile. So that decreases the smell. After decreasing the smell, we are treating the acids with sodium bicarbonate so that we are converting those assets into water soluble souls that can be washed away with soap. Thank you for watching and I hope to see you in the next video.

Key Concepts

Thiol Chemistry

Oxidation-Reduction Reactions

pH and Detergency

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