17. Acid and Base Equilibrium
Identifying Acids and Bases
Acid Identification
Most acids have one common feature and that is the presence of the hydronium ion, which is represented by H+ or H3O+.
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Identifying Binary Acids
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Hey, guys, in this new video, we're going to take a look at acids. We're going to see what are the key features that make assets acids. And, more importantly, how do we distinguish one type of acid from another? So if we take a look at the beginning, it says the most common feature of an acid is that it possesses an H plus ions. Now here's the thing. Not all acids have h plus, but a majority of them do. We're going to say the name of this H plus ions is hydro Nia, my on. Later on, we're gonna learn that certain types of acids don't possess H plus at all, but they're still assets there, just a special type of acid, which we call Lewis acids. When we get to that section, we'll cover that in detail. But for right now, just remember, most acids have H plus the stage plus ion is called hydro knee, um, ion or hydrogen ion, and we're also going to say here that H plus is the same thing as H +30 Plus. You're going to see that your professor uses them interchangeably. That's because they're the same exact thing. They're just a different rate way writing the same exact ion. So just remember, h plus is the same thing as H +30 plus. Now we're gonna say when it comes to acids, there are two major forms. Now the simpler of the two are called binary acids. Now, binary acid possesses H plus, and that H plus is connected to some electoral negative element. Now we're gonna say the electoral negative element would be nitrogen, sulfur, phosphorus or some type of halogen flooring, chlorine, bromine or iodine. Now, the key things that binary acids don't have is we're going to say no. Binary acid has oxygen. Okay, if you have oxygen on a Nass ID, that will be a different type of acid. So all binary acids, none of them have oxygen present Now, the second thing is they usually possess no medals. Usually, if we have a metal within a compound, it's Ionic, and usually it'll be base. If a metal is involved, it's usually a base off course. There are exceptions to this, and we'll talk about that later on. Now we're gonna say here the most common types off these particular acids our culture hallow acids. Hala means that we have a halogen. And of course, as it is H plus. So remember the halogen Zahren Group seven A. And if you're in group 78 What's your charge? Hopefully, you guys remember the charge distribution in the periodic table. So remember if your in group seven of your charges minus one. So we have f minus C l minus br minus. I minus. So when we have a positive h plus, connecting with one of these negative ions are are hallow acids. Would be h f hcl hbr h I. So these are your four hallow assets? Ah, hydrogen connected to a halogen. Now we could talk about other types of common binary acids based on groups, so we just looked at group seven A. So that would be HF hcl hbr h. I remember. We also have groups. Six a involved. Remember when your group six A. Your charges are negative too. So we're gonna skip oxygen and group six day, because again, binary acids don't possess any oxygen. So if you go down Group six A and you're looking at a periodic table, the next one would be as to minus s e tu minus t e tu minus. And again, these guys air combining with h plus to give us a binary acid. So let's just re remember what we learned about ionic compounds. How do we make them into compounds? Remember the charges? The number from the charges crisscross to give us our compound. Okay, so we have hte us h two s e h to t. So these will be your binary acids that are common to group six A. And then we could say that we have certain ones that are a little bit different. So these are the odd ones that they're they're technically still binary answers. They're just a little bit different. So here we could have a chat. And three And here we could have a church, CNN. So those would be the odd ones out there a little bit different from group 78 and 68 But they're still binary assets because we here we have hpe plus connected to a negative ion. And here we have hpe plus connected toa Upali, atomic ion cnegative, Cyanide ion. Now we'll learn how to name these later on and coming videos. But for right Now, these are typical, uh, common types of binary acids from groups. Six a group 78 and also the odd ones. Now that we've seen this first type of acids, it's time to talk about the second type.
Binary acids can be identified by the fact that they all possess an H+ ion attached to an electronegative element.
Oxyacids can be identified by the fact that they all possess an H+ ion connected to a nonmetal and oxygen, hence the prefix “oxy”.
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Identifying Oxyacids
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Now we're gonna say the second type. They're called oxy acids. And from the name Oxy, you could tell that it has one particular element in their oxygen. So we're gonna say oxy acids are acids that contain H plus I on. Of course, they contain oxygen, and they contained some type of nonmetal. Okay, So the difference between binary and Oxy is that Oxy has oxygen's involved. Binary does not. Something else they both share in common is that they usually do not possess any medals. Again, we're gonna see usually when we have a metal involved, that compound will be a base. Now, we're gonna say that oxy acids are formed when we hydrate non metal oxides. So in this example, here are non metal oxide would be carbon dioxide here and here would be sulfur try oxide. Okay, So non metal oxide just means you have a non metal connected to oxygen. Now all that's gonna happen is the water is going to attach itself to this whole compound. And what we get are two types off oxy acids and their oxy acids. Because both have h both have oxygen. Remember that H is really age plus they both have oxygen, and they both have some type of nonmetal involved. And that's what makes them both oxy acids. So here we would have carbonic acid. And here we have sulfuric acid. And again, we'll learn how to name these particular types of acids later on. But for right now, just realize, how do we create oxy acids? We just add H plus to some type of non metal oxide Co two s +02 s, +03 Those types of compounds, uh, P +03 Those are the kinds of compounds you add water to to make your new types of oxy acids. Now that you guys have seen the two types of assets binary and oxy, I want you guys to try to answer the next following question here. I say which the following compound or compounds cannot be classified as an acid. I gave you just brief description on on both, but try to use your best judgment to determine which one could be in which ones could not be. Then, once you're done with that click on the explanation button, you'll see a video of me explaining how to approach this problem. Guys, good luck
They are created by the hydration of nonmetal oxides.
Conversely, metal oxides create bases when hydrated by water.
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Problem
ProblemWhich of the following compound(s) cannot be classified as an acid?
A. H2S
B. HCN
C. H2
D. C2H6
E. All are acids
A
A and B
B
A and C
C
C and D
D
B and C
E
All are acids
Binary Acid Strength
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Acids and Electrolytes
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we talked about there being two classes of assets. There are binary acids and then there are oxy acids for binary acids will go over the different rules that are associated with determining the strengths of different binary acids. Binary acids have their own set of rules. Oxy acids which are a different type of acid will have their own separate list of rules that we follow for them when we're trying to compare the strengths of different oxy acids. Now, regardless if you're looking at a oxy acid or binary acids, we're gonna say strong acids in general are strong electrolytes. So they they ionized completely in water. Here we have hcl which is a strong binary acid. We have a single error going forward to show that it completely ionized it, it goes to completion. So that means we're gonna make 100% of both of these ions, weak acids are weak electrolytes. And again, whether it be weak oxy acids or weak binary acids, weak acids in general are weak electrolytes. So they don't completely ionized in water here, we don't have a solid arrow going forward, we have double arrows to say that instead of going to completion, our reaction reaches an equilibrium. So we're gonna say an equilibrium is established. So that means we're gonna make less than 100% of these ions. And in fact we tend to make a very small amount of these particular ions. So when it comes to weak acids, we're gonna have to basically set up what are called ice charts later on in order to determine the ph of these different types of weak acids. Now, when we're gonna talk about binary acids, keep in mind again, there are two classes of acids. These are just the rules for binary acids. When we talk about oxy acids, they have their own separate list of rules.
Strong Acids are strong electrolytes that completely dissociate into ions when dissolved in water.
Weak acids are weak electrolytes that don’t completely ionize, but instead reach a state of equilibrium.
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concept
Strength of Binary Acids
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here we can say that the strength of a binary acid is based on the electro negativity, which I'll abbreviate as Ian or size, which is really the atomic radius, which I'll abbreviate as they are. Of the non note. Now, remember we're looking at a periodic table as we head towards the top right corner of the periodic table, the electro negativity will increase and our atomic radius world decrease. Now when it comes to the periodic table, we don't give electro negative values to the noble gasses. Flooring is the most electro negative element on the periodic table, with a value of four point up. Now, for elements in the same period or row, then we look at their electro negativity. We're going to say here, the greater the electro negativity than the more acidic the acid. So let's say for example, I'm comparing CH four, B, H 3 & H. F. So if we look here, B, C and F, they're all in the same roar period with one another. And we would say here the greater the electron activity. The more acidic, boring we just said is the most electro negative element on the periodic table. So a check would be the most acidic out of these three options. Now, if they're in the same in the same group or column, then instead we look at their size, we're gonna say the bigger or the greater greater the atomic radius than the more acidic. So let's say we were comparing hcl hbr and H I. So C A B. R. And I as we go up the group, the atomic radius gets smaller. So you become less acidic i is larger than BR and Cl because it's lowered down the group since it's larger, it's more acidic. So H. I would be the strongest asset out of these three. Alright. So if they're in the same row, we look at electro negativity. If they're in the same group, then we look at size. But let's say they're not in the same group or ro what do we do that? Well, if they're separated by only one row from each other, then we look at their electro negativity. Alright, so how do we do something like that? Let's say we're looking here at Mm Let's say we're looking here at NH three versus H. To us. So N. Is here as is here they're not in the same role when they're not in the same group. We look at electronic activity, nitrogen is more electro negative than sulfur. You don't recall that. Make sure you go back and take a look at my video dealing with the periodic trend of electro negativity. So as a result of this, this should be a little bit more acidic than this. Now, let's say that they're separated by more than one role from each other. If they're separated by more than one role from each other, Then we're going to say here that we look at size. Okay, so let's say we're comparing let's see we're comparing NH three versus H. Two T. They're not separated by one road from each other. This is in row two. This is all the way down here. In row four size is more important, since delirium is lowered down than nitrogen is, it's larger and therefore this would be more acidic. Alright, so just keep these trends in mind when trying to compare different binary acids to one another.
When looking at a binary acid we look at both electronegativity and size to determine their strength.
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Problem
ProblemWhich is the weakest acid from the following?
A
H2S
B
H2Se
C
H2Te
D
All would have the same acid strength.
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Problem
ProblemWhich of the following acids would be classified as the strongest?
A
CH4
B
NH3
C
H2O
D
HF
E
PH3
Oxyacid Strength
The strength of an oxyacid depends on the number of oxygen atoms and the electronegativity of the nonmetal.
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concept
The Strength of Oxyacids
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in this video, we're gonna take a look at Oxy acids strength. So we're gonna say here that the strength of Oxy acids is based on the number off oxygen's or the electro negativity of the nonmetal. We're gonna go over. When do we look at either one? So here we're gonna say the rule is the number one rule for oxy acids is if my oxy acid has two or more oxygen's than hydrogen zones, then my oxy acid is a strong acid. So if we take a look at the first one we have here h n 03 we're gonna say it's an oxy acid because it contains hydrogen, a non metal and an oxygen. Here, the number of oxygen's is three. The number of hydrogen is just one. When we subtract them, we have to oxygen's remaining. You must have a minimum of two oxygen's remaining in order to be considered a strong oxy acid. Here, it meets that requirement, so it's strong. Next one, we have fennel, so C six h five h here it has one oxygen and then it has five plus one more. That's six hydrogen. So in this one, we don't have any oxygen's remaining. Remember, we need a minimum off to oxygen's remaining to be considered a strong oxy acid, so this one doesn't meet the requirements. So it's weak. Then here we have purple MK acid. So here we have four Oxygen's. We have one hydrogen, so we have three oxygen's remaining. So we've met the minimum requirement of having at least two oxygen's left, so this one would be strong. So when it comes to Oxy acids, this is the first rule that you need to remember. You need to have a minimum of at least two more oxygen's than hydrogen to be considered a strong oxy acid. We're gonna move on to the next portion when we talk about this topic of oxy acids. But keep in mind this first important role
If your oxyacid has 2 or more oxygens than hydrogens then your oxyacid is a strong acid.
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concept
Comparing the Strength of Oxyacids
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when comparing the strengths of different oxy asses remember that if they have a different number of oxygen's than the higher than remaining oxygen's the more acidic. So let's say we're comparing nitric acid versus nitrous acid. This one when we subtract the number of oxygen by hydrogen, we have two oxygen's left. This one would have one oxygen left. So since nitric acid has more remaining oxygen, it's more acidic. But let's say if they have the same number of oxygen remaining, then we'd say the more electro negative, the nonmetal, the more acidic. So let's say for instance, we're looking here at per bronek acid versus same number versus per io take acid. They both have the same job, oxygen's remaining three. So we look at electro negativity which remember as we're heading towards the top right corner of the periodic table will increase grooming is higher up than iodine. So grooming is more electro negative and therefore per bronek acid is more more acidic than per ionic acid. Now, of course, with rules, sometimes you run into exceptions. So here we have three different illustrations here for the first one we have oxalic acid which is H two C 204. When we work out the math, we still have two oxygen's remaining and when we do the same thing with ionic acid, we still have two oxygen remaining, which would tell us it should be a strong they both should be strong oxy acids. But there are exceptions to that rule, the electro negativity of their carbon and iodine is pretty low compared to other non metals. This interferes with their acidity acidity and this is the easiest way to think about this exception because of that oxalic acid and ionic acid are weak oxy acids. Now this last one doesn't necessarily represent only this compound, but it represents a class of compounds it belongs to, which is your alfa terek species. Remember a philatelic species can be acidic or basic for the group of Alphatec species that are not strong oxy acids. Even when following the math, they will have a hydrogen and they will have a negative charge hydrogen because it can be acidic negative charge because they have the ability to be basic. So here doesn't matter that we do the math and it fits the criteria to be a strong oxi acid. It just won't be because it's an esoteric. So, remember our three exceptions are oxalic acid, biotic acid and esoteric species. So just keep these rules in mind when you're trying to compare the strength of different types of oxy acids
When comparing the strengths of different oxyacids remember:
If they have different number of oxygens then the more oxygens the more acidic
If they have the same number of oxygens then the more electronegative the nonmetal the more acidic.
With some rules there are exceptions. Oxalic acid and Iodic acid have two more oxygens than hydrogens but are weak acids because carbon are iodine have low electronegativity.
Amphoteric species (compounds that can act as both an acid or a base) are also an exception to the rule for oxyacids.
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Problem
ProblemRank the following oxyacids in terms of increasing acidity.
a) HClO3
b) HBrO4
c) HBrO3
d) HClO4
A
A< C < B< D
B
C < B < A < D
C
C < A < B < D
D
A < C < D < B
Base Strength
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concept
Bases and Electrolytes
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Hey, guys, In this new video, we're gonna finally take a look at the strength of bases. So up to this point, we've talked about acids. We've talked about binary acids and oxy acids, and we should know their strengths at this point is, Well, how do we determine when they're weak and what they're when they're strong again? This is important because weak acids, we have to use a nice chart in order to find pH strong acids. We don't have to do that. So what we're gonna say now is let's take a look at bases. We're gonna say strong bases are considered to be strong electrolytes and what a strong electrolytes mean, it means that it completely breaks up or associates when dissolved in water. Here, you're gonna notice that we have a solid era going forward again. This means reaction goes to completion, so all of the reactant will break down basically to 100%. So we get those two ions, we get an A plus O. H minus. Now, weak acids are considered to be weak electrolytes, so they don't completely break down. They don't completely ionized here again will notice that there's a double arrow, meaning that an equilibrium is established. That means our reaction goes in the four direction as well as the reverse direction. Now, Weak acids week faces favor the reactant. All that means is that our reactions really don't break down that much. So a majority of our compound will be in the form of reactant. Very little of it will be made into product in the opposite way. Strong acids and strong bases favor. We're gonna say they favor the products, which means nearly all of our react and breaks down to give us products. So again, remember weak acids week basis. We need to use a nice chart to find pH or P O. H. We'll talk about those later down the road. It's imperative that you guys remember how toe identify things.
Strong Bases are strong electrolytes that completely dissociate into ions when dissolved in water.
Weak bases are weak electrolytes that don’t completely ionize, but instead reach a state of equilibrium.
Bases are characterized by THREE major features:they may possess metals, they may have a negative charge or they may be an amine.
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concept
Bases and Group 1A
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Now, if we take a look here, we're gonna say when it comes to bases, there are three features that were supposed to look out for. Generally, bases possess medals. So from metal is involved, then it's most likely going to be a base. We're going to see a couple exceptions of that when we get to ANFO Terek species. But for right now, let's not worry about that. Next, we're gonna stay basis, tend to have a negative charge. Okay, so bases will have medals or a negative charge, or they'll be classified as another compound, which we call a means now means are or organic type of compound. But we get to see them for the first time in chemistry. So before you guys move onto organic, you get a small taste of what a means are. And how exactly do they relate to bases? So if we take a look at the rules, we're gonna say Group one A. We're gonna say any group won a medal when they combined with any one of these four ions make a strong base. Now, these four ions, we call them hydroxide ion hydrogen can be positive or negative when it's positive it's called Hydro Nia My on. But when it's negative, it's called hydride ion. 02 minuses oxide and NH two minus is a mydd. So notice all of them and with i d e. Because they have a negative charge present. So if one of these negative ion combines with any group won a medal, it's gonna create a strong base. Now recall what are the charges of Group one? A medals group 18 medals are plus one. So, examples we could have any positive ally Positive C s positive K positive. Any of these ions could react with any one of those four ions to give me a strong base. So a year and a positive O H minus combined together to give me an H. This would give me Al I h The two from here would come here. The one from here would come over here CS then here we have K and h two. Remember, you can mix and match any group. When a ion with any one of those four here we get sodium hydroxide, lithium hydride, caesium oxide, potassium hmeid. So, again, any group win a medal with one of those four ions will create a strong base, and strong bases don't require a nice chart in order to find pH or P O. H.
Any Group 1A metal when combined with OH –, H –, O2– or NH2 – makes a STRONG BASE.
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concept
Bases and Group 2A
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next, we're gonna say group to a ions. And here there are There's a caveat. It's not all group to wait. It's certain metals in group two way. So we're gonna say any group to a metal from calcium to bury him when combined with O. H minus, H minus, O to minus or an H two minus will create a strong base. So remember, if you look at your periodic table group two way, we're gonna see beryllium, magnesium, calcium, strontium, barium, and we have our And at the bottom is well, and usually we don't see basis with that, so we're not gonna worry too much about it. So we're saying from calcium and lower. Okay, so the cut off is calcium. These two get left out. So here we're gonna say Group two A is plus two in charge. So we could have these guys reacting with any one of these ions. Okay, so the two from here will come over here. The one from here will move over there cause nothing. So this would be CEO H two here. We're gonna get the to from here. Coming here. B a h two. This is plus two this is minus two. So when they combine, they cancel out, and then the two from here can come down here. So those are all examples of strong bases. Now we're going to stay here, that magnesium is above calcium, and we're gonna say magnesium hydroxide is a base now. Technically, it's a week base. It's not as strong as the others. The others break up 100%. But here's the thing about magnesium hydroxide. We're gonna say a small portion it off. It will dissolve. So let's say about 10% of it dissolves that small portion of it that does dissolve. It dissolves all the way. And when it comes to a weak acids and bases, sometimes a piece of it will dissolve, but not completely for magnesium hydroxide. A small portion of it dissolves and it dissolves completely. Because of that weirdness, we're gonna say M G. O. H. Two is not a strong base, but it's strong enough that we don't need to do a nice chart. So we're gonna say magnesium hydroxide is a weird special case. Technically, it's weak, but it's strong enough that it may not require a nice chart. Just make a little note of that
Group 2A metals, from Ca2+ to Ba2+, when combined with OH –, H –, O2– or NH2 – makes a STRONG BASE.
Amines are compounds with only nitrogen or hydrogen (i,e. NH3) or with carbon, nitrogen and hydrogen (i,e. CH3NH2).
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concept
Amines
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then finally, the last group we talked about, we're gonna say a means. And since we're gonna meet some room guys to do this, I'm gonna remove myself from the image so we have more room to work with. So it means what the heck isn't a mean what we're gonna say. Inamine is a compound that has, and an H nitrogen and hydrogen such as example, and H three. Or it's a compound that has carbon, hydrogen and nitrogen. Example of that we could have ch three NH two. Okay, so just remember, that means or compounds with nitrogen and hydrogen or carbon, hydrogen and nitrogen. We're gonna say here that neutral a means ones without charges are considered to be weak bases. Examples the two we just wrote and h three or C h three n. H. Two. Now, obviously, there are more than just these, But these air good two examples we have ammonia and then methyl amine methyl amine. The name even tells you that it's in a mean and we're gonna say next that positive, Positively charged. A means are considered to be weak acids. So here we could have NH four positive, which is ammonium. This is ammonia, so ammonium is positive. So it's a weak acid or C H three and H three positive. This would be methyl ammonium. Okay, now we saw compound earlier when we talked about binary acids. That compound was H C N. Now H. C n has the characteristics of on a mean right. I said it was carbon, hydrogen and nitrogen. But remember, you can't be a binary acid and a I mean at the same time, so H. C. And even though it has those three elements is not another mean. It's not in a mean it is a binary acid, so make note of that. This is hydro scion IQ acid, not in a mean, so just make note of that. What in the mean is it usually has just and an H or could have H CNN. HCM, though, is not in a mean it's a binary acid. So look out for those characteristics. And if they give you the name, usually you'll see a meaning the name in some way. That will be a clear giveaway that you're dealing with in a mean now. Hopefully, guys have learned how to identify acids and bases now because again, it's imperative that you know how to identify them as either weak or strong, because if you don't know that, you won't know how to calculate pH or anything else dealing with acid base chemistry.
Neutral Amines are considered weak bases.
Positive Amines are considered weak acids.
15
example
Classify each of the following as a strong acid, weak acid, strong base or weak base
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Hey, guys, in this new video, we're gonna put to practice some of the concepts we learned dealing with acids and bases. How doe identify them. And are they weak, or are they strong? So in this first example, it says, classify each of the following as a strong acid, a weak acid, a strong base or a week base. So remember, this is what we're gonna do. This is the protocol to follow when figuring out if something is an acid or base. First, we're gonna ask ourselves some important questions. First, let's identify if it's a base. We're going to say one. Does it have a metal for the first one? It doesn't have a medal to Doesn't have a negative charge anywhere. We don't see a negative charge. Three. Is it gonna mean remember, And a mean has H and N or H C and N doesn't have those lineups, so it's not in a mean. So that means they could not possibly be a base, so that means it's an acid. Is that a binary acid, or is it an oxy acid? If it has oxygen in it, it's a oxy acid, so we know it's not a base. So it has to be an oxy acid because of these oxygen's. We know it's an oxy acid, so let's just do the rules to determine if it's weak or strong. So remember, we look at the number of oxygen's we have to oxygen's minus two hydrogen, leaving us with nothing left. Remember, we need a minimum of two oxygen's left if we don't have that minimum. Couldn't be a strong acid, so this would be a week. Oxy acid. Next, let's go to C. We have H two N N H to ask ourselves the question. Does it have a metal? No. Does it have a negative charge? No. Is it in a mean Remember A means have H and end just like that compound. It has only H and N. Therefore, it isn't a mean. All you say now is Is it positive or is it neutral? It's a neutral, mean and neutral means are weak bases. So this particular week basis called hydrazine to so here. We're going to say this is a week base because it's a neutral amine. Next one be. Does it have a metal? No. Does it have a negative charge? No. Is it in a mean? It has a ches. It has carbon and it has a nitrogen, so it's definitely a mean. Now we just ask ourselves, Is it positive or is it neutral? Since it's positively charged and they will tell you? Since it's positively charged, it's in a mean it's a positive. I mean, so it must be a weak acid. And indeed, the last one. Does it have a medal? No. Does it have a negative charge? No. Is it in a mean? Does it have a Chand N? Nope. Does it have HC N? Nope. So it's an acid. If it has oxygen, it's an oxy acid. Here it has oxygen, so it's definitely an oxy acid. Let's do the math. Three. Oxygen's minus one hydrogen gives us to Oxygen's left. Definitely a strong oxy acid. So that's the protocol I want you guys to follow. We have more practice to do. I want you guys to attempt to do practice. Question one. Ask yourselves the questions. Does it have a medal? Does it have a negative charge? If it is it in a mean If Noda all three, then it's an acid. If it has no oxygen. It's a binary. If it does have oxygen, it's an oxy. And if we go back to bases, if it has a metal, remember, if it has a metal, what are the four ions it has to be connected to? To be a strong base. Say that to yourself if it if it's negative, Ion is not one of those four, um, ions that make it a strong base. Then it's a week base. So guys attempted to practice. Question went on your own. Come back, click on the explanation button and see what the answers are and how I determine them. Good luck.
16
Problem
ProblemClassify each of the following as a strong acid, weak acid, strong base or weak base.
A
B
C
D
17
Problem
ProblemClassify each of the following as a strong acid, weak acid, Strong base, or weak base.
A
B
C
D
18
Problem
ProblemClassify each of the following as a strong acid, weak acid, strong base or weak base.
A
B
C
D
Additional resources for Identifying Acids and Bases
PRACTICE PROBLEMS AND ACTIVITIES (182)
- The following pictures represent equal volumes of aqueous solutions of three acids HA (A = X, Y, or Z); water...
- Consider the conjugate bases, 1X-, Y-, Z-2 in Problem 2. If you mix equal concentrations of reactants and pro...
- Which is the strongest acid? (LO 16.4) (a) HClO3 (b) HBrO3 (c) H2SO3 (d) H2TeO3
- The probe of the pH meter shown here is sitting in a beaker that contains a clear liquid. (c) Why is the tempe...
- What is the concentration of hydroxide ions 3OH-4 in a glass of wine with pH = 3.64? (LO 16.5, 16.6) (a) 2.3...
- The following diagrams represent aqueous solutions of three acids, HX, HY, and HZ. The water molecules have be...
- The following diagrams represent aqueous solutions of three acids, HX, HY, and HZ. The water molecules have be...
- An acid solution with a concentration of 0.500 M has a pH = 3.21. What is the Ka of the acid? (LO 16.8) (a) ...
- Each of the three molecules shown here contains an OH group, but one molecule acts as a base, one as an acid, ...
- Phenylephrine, an organic substance with molecular formula C9H13NO2, is used as a nasal decongenstant in over-...
- Phenylephrine, an organic substance with molecular formula C9H13NO2, is used as a nasal decongenstant in over-...
- Ammonia 1NH32 has base dissociation constant 1Kb2 of 1.8 * 10-5. What is the concentration of an aqueous ammo...
- Consider the molecular models shown here, where X represents a halogen atom. (b) Does the acidity of each mole...
- Consider the molecular models shown here, where X represents a halogen atom. (a) If X is the same atom in both...
- Which of the following statements is false? (a) An Arrhenius base increases the concentration of OH- in water...
- Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+.
- Give the conjugate base of the following Brønsted–Lowry acids: (i) HCOOH, (ii) HPO42-.
- Give the conjugate acid of the following Brønsted–Lowry bases: (i) SO42-, (ii) CH3NH2.
- (a) Calculate the percent ionization of 0.0075 M butanoic acid 1Ka = 1.5 * 10-52.
- (b) Calculate the percent ionization of 0.0075 M butanoic acid in a solution containing 0.085 M sodium butanoa...
- Identify the Brønsted–Lowry acid and the Brønsted–Lowry base on the left side of each of the following equatio...
- (a) Calculate the percent ionization of 0.125 M lactic acid 1Ka = 1.4 * 10-42.
- Identify the Brønsted–Lowry acid and the Brønsted– Lowry base on the left side of each equation, and also iden...
- What is the conjugate acid of HSO3-? What is its conjugate base?
- Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In eac...
- Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In eac...
- Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In eac...
- Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In eac...
- Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In eac...
- Label each of the following as being a strong acid, a weak acid, or a species with negligible acidity. In each...
- Predict the products of the following acid–base reactions, and predict whether the equilibrium lies to the lef...
- You are asked to prepare a pH = 3.00 buffer solution starting from 1.25 L of a 1.00 M solution of hydrofluori...
- You are asked to prepare a pH = 4.00 buffer starting from 1.50 L of 0.0200 M solution of benzoic acid 1C6H5COO...
- Predict the products of the following acid–base reactions, and predict whether the equilibrium lies to the lef...
- A formic acid solution has a pH of 3.25. Which of these substances will raise the pH of the solution upon addi...
- Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. b. a solution that i...
- Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. a. a solution that i...
- Calculate 3H+4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neu...
- Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or ne...
- Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or ne...
- Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or ne...
- Calculate the percent ionization of a 0.15 M benzoic acid solution in pure water and in a solution containing...
- Which of the following solutions is the most acidic? (a) 0.2 M Ba(OH)2, (b) 0.2 M H2SO3, (c) 1.0 M glucose 1C...
- Which of the following solutions is the most basic? (a) 0.6 M NaCl, (b) 0.150 M CsOH, (c) 0.100 M Sr1OH22.
- Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. c. a mixture that is...
- Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. b. 0.15 M NaF
- Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. a. 0.15 M HF
- By what factor does 3H+4 change for a pH change of (a) 2.00 units?
- State whether each of the following statements is true or false. Justify your answer in each case. (c) Metha...
- State whether each of the following statements is true or false. Justify your answer in each case. (b) HCl i...
- In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conju...
- In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conju...
- In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conju...
- Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the sub...
- Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the sub...
- Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the sub...
- In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conju...
- In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conju...
- Write the formula for the conjugate base of each acid. d. HF
- Write the formula for the conjugate base of each acid. c. HCHO2
- Write the formula for the conjugate base of each acid. b. H2SO3
- The average pH of normal arterial blood is 7.40. At normal body temperature 137 °C2, Kw = 2.4 * 10-14. Calcula...
- Write the formula for the conjugate base of each acid. a. HCl
- Write the formula for the conjugate acid of each base. c. HSO4
- The following pictures represent aqueous solutions of three acids HA1A = X, Y, or Z2; water molecules have be...
- The following pictures represent aqueous solutions of three acids HA1A = X, Y, or Z2; water molecules have bee...
- Locate sulfur, selenium, chlorine, and bromine in the periodic table: (a) Which binary acid 1H2S, H2Se, HCl, ...
- Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constan...
- Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constan...
- Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constan...
- Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constan...
- Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constan...
- Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constan...
- Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constan...
- The following pictures represent solutions of three salts NaA (A- = X-, Y-, or Z-); water molecules and Na+ io...
- The following pictures represent solutions of three salts NaA (A- = X-, Y-, or Z-); water molecules and Na+ io...
- The following picture represents the hydrated metal cation M1H2O26 n + , where n = 1, 2, or 3. (c) Which ...
- Pick the stronger base from each pair. c. F- or ClO-
- Calculate [H3O+] and [OH-] for each solution at 25 °C. b. pH = 11.23
- Calculate [H3O+] and [OH-] for each solution at 25 °C. a. pH = 8.55
- Complete the table. (All solutions are at 25 °C.)
- Complete the table. (All solutions are at 25 °C.)
- Phenylacetic acid 1C6H5CH2COOH2 is one of the substances that accumulates in the blood of people with phenylk...
- A 0.100 M solution of chloroacetic acid 1ClCH2COOH2 is 11.0% ionized. Using this information, calculate 3ClC...
- A 0.100 M solution of bromoacetic acid 1BrCH2COOH2 is 13.2% ionized. Calculate 3H+4, 3BrCH2COO-4, 3BrCH2COOH4...
- The hydronium ion H3O+ is the strongest acid that can exist in aqueous solution because stronger acids dissoc...
- Calculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH of an aci...
- If a solution of HF 1Ka = 6.8 * 10-42 has a pH of 3.65, calculate the concentration of hydrofluoric acid.
- Determine the concentration of H3O+ to the correct number of significant figures in a solution with each pH. ...
- Which acid in each of the following pairs has the stronger conjugate base? See Table 16.1 to compare the relat...
- The acid-dissociation constant for chlorous acid 1HClO22 is 1.1 * 10-2. Calculate the concentrations of H3O+, ...
- Which base in each of the following pairs has the stronger conjugate acid? See Table 16.1 to compare the rela...
- Arrange each group of compounds in order of increasing acid strength. Explain your reasoning. (a) HCl, H2S, PH...
- Determine the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (c) 0.165 M hy...
- The pH of a solution of NH3 and NH4Br is 8.90. What is the molarity of NH4Br if the molarity of NH3 is 0.016 M...
- Calculate the percent dissociation of 0.10 M hydrazoic acid (HN3, Ka = 1.9 X 10^-5). Recalculate the percent d...
- Would you expect zirconium(II) oxide, ZrO, to react more readily with HCl(aq) or NaOH(aq)?
- Calculate the pH of 100.0 mL of 0.30 M NH3 before and after the addition of 4.0 g of NH4NO3, and account for t...
- Arrange the following oxides in order of increasing acidity: K2O, BaO, ZnO, H2O, CO2, SO2.
- Identify the weakest acid in each of the following sets. Explain your reasoning. (b) NH3, H2O, H2S
- Identify the weakest acid in each of the following sets. Explain your reasoning. (a) H2SO3, HClO3, HClO4
- Chlorine reacts with oxygen to form Cl2O7. (c) Would you expect Cl2O7 to be more reactive toward H+1aq2 or OH...
- Calculate the percent ionization of propionic acid 1C2H5COOH2 in solutions of each of the following concentrat...
- An element X reacts with oxygen to form XO2 and with chlorine to form XCl4. XO2 is a white solid that melts at...
- An element X reacts with oxygen to form XO2 and with chlorine to form XCl4. XO2 is a white solid that melts at...
- Citric acid, which is present in citrus fruits, is a triprotic acid (Table 16.3). (a) Calculate the pH of a 0....
- Determine the pH of an HNO2 solution of each concentration. In which cases can you not make the simplifying as...
- Write balanced equations for the following reactions: (a) boron trichloride with water
- Write balanced equations for the following reactions: (c) phosphorus pentoxide with water
- Determine the pH of an HF solution of each concentration. In which cases can you not make the simplifying assu...
- Write balanced equations for the following reactions: (d) arsenic trioxide with aqueous potassium hydroxide.
- Consider the base hydroxylamine, NH2OH. (a) What is the conjugate acid of hydroxylamine?
- A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (Ka) for the a...
- Determine the percent ionization of a 0.125 M HCN solution.
- Determine the percent ionization of a 0.225 M solution of benzoic acid.
- Ephedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a w...
- Ephedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a w...
- Calculate the percent ionization of a formic acid solution having the given concentration. d. 0.0500 M
- Calculate the percent ionization of a formic acid solution having the given concentration. c. 0.100 M
- Calculate the percent ionization of a formic acid solution having the given concentration. b. 0.500 M
- Calculate the percent ionization of a formic acid solution having the given concentration. a. 1.00 M
- Codeine 1C18H21NO32 is a weak organic base. A 5.0 * 10-3M solution of codeine has a pH of 9.95. Calculate the...
- A 0.148 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid ionization cons...
- Calculate the H3O+ concentration to the correct number of significant figures for solutions with the following...
- Calculate the H3O+ concentration to the correct number of significant figures for solutions with the followin...
- Find the pH of each mixture of acids. a. 0.115 M in HBr and 0.125 M in HCHO2
- Which of the following species behave as strong acids or as strong bases in aqueous solution? (a) HNO2 (b) HNO...
- Using data from Appendix D, calculate 3OH-4 and pH for each of the following solutions: (b) 0.035 M Na2S
- Pyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqu...
- Pyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqu...
- The value of Ka for nitrous acid 1HNO22 at 25 °C is given in Appendix D. (a) Write the chemical equation for t...
- Predict the stronger acid in each pair: (e) benzoic acid (C6H5COOH) or phenol (C6H5OH).
- Predict the stronger acid in each pair: (c) HBrO3 or HBrO2
- Look up the values of Ka in Appendix C for C6H5OH, HNO3, CH3CO2H, and HOCl, and arrange these acids in order ...
- Determine the [OH-], pH, and pOH of a 0.15 M ammonia solution.
- Based on their compositions and structures and on conjugate acid–base relationships, select the stronger base ...
- Based on their compositions and structures and on conjugate acid–base relationships, select the stronger base ...
- Indicate whether each of the following statements is true or false. For each statement that is false, correct ...
- Caffeine (C8H10N4O2) is a weak base with a pKb of 10.4. Calculate the pH of a solution containing a caffeine c...
- Amphetamine (C9H13N) is a weak base with a pKb of 4.2. Calculate the pH of a solution containing an amphetami...
- Indicate whether each of the following statements is true or false. For each statement that is false, correct ...
- Morphine is a weak base. A 0.150 M solution of morphine has a pH of 10.7. What is Kb for morphine?
- A vitamin C tablet containing 250 mg of ascorbic acid 1C6H8O6; Ka = 8.0 * 10-52 is dissolved in a 250 mL glas...
- Acetic acid 1CH3COOH; Ka = 1.8 * 10-52 has a concentration in vinegar of 3.50% by mass. What is the pH of vi...
- Determine the [OH-] and pH of a solution that is 0.140 M in F-.
- Indicate whether each of the following statements is correct or incorrect. (c) Conjugate acids of weak bases p...
- A typical aspirin tablet contains 324 mg of aspirin (acetylsalicylic acid, C9H8O4), a monoprotic acid having ...
- Write balanced net ionic equations and the corresponding equilibrium equations for the stepwise dissociation ...
- Determine the pH of each solution. a. 0.10 M NH4Cl
- Calculate the concentration of all species in a 0.15 M KF solution.
- Calculate the concentration of all species in a 0.225 M C6H5NH3Cl solution.
- Write chemical equations and corresponding equilibrium expressions for each of the three ionization steps of ...
- Butyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (c) Calculat...
- Butyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (b) Calculat...
- Calculate the [H3O+] and pH of each polyprotic acid solution. a. 0.350 M H3PO4
- Ritalin is the trade name of a drug, methylphenidate, used to treat attention-deficit/hyperactivity disorder i...
- Strychnine 1C21H22N2O22, a deadly poison used for killing rodents, is a weak base having Kb = 1.8 * 10-6. Cal...
- What is the pH at 25 C of water saturated with CO2 at a partial pressure of 1.10 atm? The Henry's law constan...
- The amino acid glycine 1H2N¬CH2¬COOH2 can participate in the following equilibria in water: H2N¬CH2¬COOH + H2O...
- Oxycodone 1C18H21NO42, a narcotic analgesic, is a weak base with pKb = 5.47. Calculate the pH and the concent...
- Based on molecular structure, arrange the binary compounds in order of increasing acid strength. Explain your...
- In nonaqueous solvents, it is possible to react HF to create H2F+. Which of these statements follows from thi...
- Based on molecular structure, arrange the oxyacids in order of increasing acid strength. Explain your choice....
- Which is a stronger base, S2 - or Se2 -? Explain.
- Write a balanced net ionic equation for the reaction of each of the following ions with water. In each case, i...
- Based on these molecular views, determine whether each pictured acid is weak or strong.
- Calculate the concentrations of all species present and the pH in 0.10 M solutions of the following substance...
- Calculate the pH and the percent dissociation of the hydrated cation in 0.020 M solutions of the following su...
- Calculate the pH and the percent dissociation of the hydrated cation in the following solutions. See Appendix ...
- The AIDS drug zalcitabine (also known as ddC) is a weak base with a pKb of 9.8. What percentage of the base is...
- The pH of a 1.00 M solution of urea, a weak organic base, is 7.050. Calculate the Ka of protonated urea.
- Lactic acid is a weak acid found in milk. Its calcium salt is a source of calcium for growing animals. A satur...
- Calculate the pH and the concentrations of all species present (H3O+ , F-, HF, Cl-, and OH-) in a solution th...
- When NO2 is bubbled into water, it is completely converted to HNO3 and HNO2: 2 NO21g2 + H2O1l2S HNO31aq2 + H...
- Acid and base behavior can be observed in solvents other than water. One commonly used solvent is dimethyl s...
- A 7.0 mass % solution of H3PO4 in water has a density of 1.0353 g/mL. Calculate the pH and the molar concentra...
- In qualitative analysis, Ca2+ and Ba2+ are seperated from Na+, K+, Mg2+ by adding aqueous (NH4)2CO3 to a solut...
- In the case of very weak acids, 3H3O+ 4 from the dissociation of water is significant compared with 3H3O+ 4 ...
- In aqueous solution, sodium acetate behaves as a strong electrolyte, yielding Na+ cations and CH3CO2 - anion...
- A 1.000 L sample of HF gas at 20.0 °C and 0.601 atm pressure was dissolved in enough water to make 50.0 mL of...
- A 1.000 L sample of HF gas at 20.0 °C and 0.601 atm pressure was dissolved in enough water to make 50.0 mL of...
- You may have been told not to mix bleach and ammonia. The reason is that bleach (sodium hypochlorite) reacts ...