00:02 Good day, everyone.

00:14 My name is Charles Christopher.

00:17 I'm the chemistry teacher,

00:18 and I'll be taking you on the topic,

00:20 all sides of carbon.

00:23 Now, before I begin,

00:25 I would like to give you some of the objectives

00:28 of the class.

00:30 Now, at the end of the class,

00:33 the students should be able to know,

00:36 basically, the oxides of carbon, all right,

00:41 which are the carbon two oxides and the carbon four oxides.

00:44 The basically, it should be able to know

00:46 the preparation of carbon.

00:48 Our carbon can be prepared in laboratory.

00:50 That's carbon two oxides,

00:51 I mean, all sides of carbon can be prepared in the laboratory.

00:53 So, the carbon two oxides and carbon four oxides.

00:57 So, now, basically, we wanna talk about carbon two oxides.

01:01 Now, first of all, we're picking carbon two oxides first.

01:04 Now, carbon two oxides, basically,

01:06 is actually a form of carbon,

01:09 oxides of carbon that is formed

01:12 with carbon bonds in limites or plough of air.

01:17 So, we also call it carbon monoxide, basically, all right?

01:22 It's called carbon monoxide,

01:23 because the velocity of oxygen there is actually two.

01:28 All right, when you calculate the velocity of oxygen

01:32 in carbon two oxides, so you have two.

01:36 Okay, that is why it's called carbon two oxides, basically.

01:39 So, now, carbon exhibits, like I said,

01:42 variable or digital state, like you have in metals.

01:46 So, you can exist as an eta two or four, all right?

01:51 So, when you make use of the two,

01:53 so, of course, when you do the calculation,

01:54 at the end of the day, you'll find out that for two,

01:58 so, the compound, it will form when it bonds in air,

02:01 when carbon bonds in air.

02:03 So, you're gonna have a carbon two oxides.

02:05 They're when you use that four.

02:06 So, when carbon bonds in air,

02:08 with the edge of the village in between carbon and oxygen,

02:11 so, you're gonna have a carbon four oxides.

02:13 But first, we are looking at carbon two oxides,

02:16 as a case would be, okay?

02:17 So, then, now, carbon monoxide is actually

02:19 colorless and odorless, all right?

02:22 And it tastes less, it tastes less gas,

02:25 that is slightly less dense than air, okay, as we know.

02:30 Now, how do we prepare these carbon two oxides in the laboratory?

02:34 So, now, there are different methods we use here.

02:36 So, I'm gonna actually show you how we can use

02:39 the different method to prepare carbon two oxides in the laboratory.

02:43 Now, for the first method,

02:46 so, a carbon two oxides, sorry, which is also known as carbon monoxide,

02:50 is prepared in the laboratory by the hydroxane metanoid acid.

02:55 So, when metanoid acid is dehydrated.

02:57 Now, what is dehydration?

02:58 The dehydration is simply removing molecules of water,

03:02 or the adjozoid that you're from, that particular substance.

03:04 So, removing the acute group from that part,

03:10 or the constant, substance that is constant here, all right?

03:13 For here, the metanoid acid is also known as formic acid, okay?

03:18 Take notes of that.

03:19 So, that when you dehydrate these,

03:21 naturally, dehydration means something has water removed,

03:27 that's dehydration, okay?

03:29 So, we're gonna remove the water molecule for metano

03:31 to see what the result would be.

03:33 So, of course, at the end of the day,

03:34 we're gonna have carbon two oxides.

03:37 So, then now, you can also use, apart from using metanoid acid,

03:43 you can also use a dead direct acid,

03:45 which is a zallic acid, all right?

03:47 So, now, for this case, we have to pass a true carbon,

03:52 two or four oxides, which is carbon dioxide, okay?

03:56 True red hotel carbon, okay?

03:59 So, for the dehydration, basically,

04:01 what happens if I've explained this already into you?

04:04 What happens here, basically, is,

04:06 for it to actually be passed through a dehydrated agent.

04:10 So, the dehydrated agent, we use mostly here, it's H2SO4, okay?

04:14 So, what we use, so as you can see,

04:16 this equation here.

04:17 So, do you can dehydrate this?

04:19 What does it mean?

04:20 I told you, dehydration means removing molecules of water.

04:24 So, if, here now, I remove this part,

04:29 they remove this part from this place.

04:31 So, what does the removing exist, particular one?

04:36 All right, remove the molecules of water

04:38 from this, what's it called, the metanoid calcium?

04:42 So, at the end of the day,

04:43 you are going to have carbon two oxides.

04:45 So, as you can see, in this equation,

04:47 so, carbon two oxides, it's actually from here,

04:49 alongside with water, okay?

04:52 So, now, that's for that.

04:55 Now, another thing, of course, with the diagram,

04:58 you can actually see how this is done.

05:00 Now, don't forget that the dehydration agent,

05:02 we use the H2SO4, the H2SO4 must be a concentrated form.

05:06 So, of course, you can see this diagram explaining

05:09 how this process is actually done.

05:11 Of course, time will fail me to actually show you

05:13 the various stages we do here.

05:16 Of course, this one is actually your delivery tube.

05:19 All right, this is your delivery tube.

05:20 Then, why this one is your round bottom,

05:23 sorry, about that.

05:24 This one is your round bottom flask.

05:26 All right, as you can see.

05:28 So, now, the formic acid here,

05:31 which is metanoid acid here,

05:33 is actually transfer into this round bottom flask.

05:36 What happened here is that.

05:37 Now, forget this one, it takes so far now.

05:39 You see the shape of the funnel here?

05:40 This one, you know, we have different types of funnel, okay?

05:43 So, we have invited for now,

05:44 our TSO4 now, we have a glassy funnel,

05:48 we have different types of funnel.

05:49 So, but this one, the type of funnel

05:50 we use is called TSO4 now, all right?

05:53 Now, the formic acid is transferred

05:57 through the TSO4 now into this round bottom flask.

05:59 What happened here is that the concentrated sulfuric acid

06:03 is also passing to the same round bottom flask

06:05 to help to dehydrate it,

06:07 because it's a dehydrated agent, all right?

06:09 To remove molecules of water from it.

06:12 Then, after that, when a carburetor oxide is formed,

06:15 the carburetor oxide is passed through the delivery tube

06:18 into this water, this is a water on pneumatic trough.

06:23 So, pneumatic trough has a gas jar standing on it.

06:27 So, that is the gas jar that has been evacuated, okay?

06:30 So, where, of course, we collect our carbon monoxide from it.

06:34 So, basically, we can also use that mix too,

06:37 apart from that metanoic acid,

06:39 we can also use ethythic dioxide.

06:43 Ethythic dioxide is heated warmly with the concentrated,

06:47 the same concentrated sulfur, all right?

06:49 Basically, to form a gaseous mixture of cotton,

06:52 equal amount of carburetor oxide and carbon monoxide,

06:57 I mean, carburetor oxide, all right?

06:59 And don't forget here, what we are looking for here

07:02 to take is carburetor oxide.

07:04 But alongside, carburetor oxide is also formed.

07:07 Like you can see in this equation here,

07:09 this equation is showing us how that happens.

07:12 So, then this one is a ethythic dioxide.

07:15 So, that is actually be dehydrated

07:18 by conch issue, so forth, to form carburetor oxide

07:22 and carburetor oxide, basically.

07:24 So, this is diagram also explaining that in fact.

07:28 But the difference between that first diagram,

07:30 this one is the et between, this one has potassium hydrozide.

07:35 What the positive solution does is to help to dry the carburetor oxide,

07:41 all right, that is formed along the way, okay?

07:44 Then thereby, it's be collected here

07:47 through a delivery tube, okay?

07:49 So, as you can see here,

07:50 then be collected from this gas jar here, as you can see here.

07:53 So, now, last quantity of carburetor oxide, all right?

07:56 is produced by a copy convoxial of carbure compounds

08:00 like Petru, like we have a, basically Petru generally, okay?

08:05 But there are other examples also as well.

08:09 So, but the obtain, which is a CH, CH18, all right,

08:14 which is the obtain, now that's a chemical formula

08:18 for the components of Petru, that bonds

08:21 in the presence of oxygen, all right,

08:23 to give, to actually, like, greater water,

08:27 and form large quantity of our carbon monuzer,

08:30 as you can see, this equation here, all right,

08:32 that is explaining this, that in fact, too.

08:34 So, we're also using the metal of reduction,

08:37 reduction process.

08:38 So, of course, you know what reduction is, all right?

08:42 Carbon for oxide is prepared in the laboratory, all right?

08:46 By using metal of reduction, okay?

08:50 So, this is actually done through the reaction

08:53 from marble chips, okay?

08:55 With diluted hydrochloric acid, okay?

08:58 Now, basically, the carburetics,

09:00 that is then passed through strongly heated charcoal,

09:04 where it is mostly reduced to carbon monoxide, okay?

09:09 That's another way of producing the carbon monoxide,

09:12 as well as just like you can see it in this equation here,

09:15 all right, basically.

09:16 So, but the CO gas that is actually,

09:19 that is further passed, that is formed,

09:22 is further passed through concentrated sodium hydroxide,

09:25 like you can see in between,

09:27 in that diagram, I just illustrated,

09:29 we can see that.

09:30 So, to remove the acopniate carbon for oxide,

09:32 so, the carbon for oxide has to be removed,

09:34 because that's not not part of what we are looking for.

09:37 So, we are actually looking for carbon monoxide, okay?

09:39 So, that carbon for oxide is removed

09:42 by passing it through concentrated sodium hydroxide,

09:44 okay, to remove it.

09:46 Now, basically, finally, what we now have is

09:49 the PO carbon two oxide,

09:51 which is actually collected over,

09:53 that gas gas is the, we have it in the diagrams,

09:58 like the one I showed you the two diagrams,

10:00 for the two processes that we have,

10:02 as the hydration process and the reduction method

10:07 of the pericabal two oxides.

10:09 So, now, let's now look at the properties of carbon two oxides,

10:13 basically, for the problem of carbon two oxides,

10:15 it's colorless, of course, you know that, all right?

10:18 Almost the colorless, most times, you call it colorless,

10:22 basically, I mean, almost all the less.

10:24 That is, that's no smell, okay?

10:27 So, it's taste less, as well.

10:28 It's a taste less gas, does not have taste.

10:31 So, it is slightly lighter than here, all right?

10:34 So, we know that, so this vapor density is actually 14.

10:37 So, is this highly poisonous?

10:39 Of course, we know that.

10:40 So, just like, you can't actually keep inside the room

10:43 where people are and everywhere is closed.

10:46 There's no ventilation.

10:47 So, people there, we actually that of that carbon monosa,

10:51 because it's very poisonous.

10:52 So, now, the air containing even less than 1% of carbon monosa,

10:56 okay, can be fatal.

10:58 Very, in fact, just 1% of it can be very dangerous of it, okay?

11:03 When you breathe in, for about 10 to 15 minutes,

11:06 the person can eventually, that.

11:08 So, the chemical properties of carbon monosa is that,

11:12 it has to do with combination reaction most times.

11:16 So, combination reaction, you know what we're talking about?

11:18 Combination of constituents, elements.

11:20 So, basically, like we have it here,

11:22 combination with oxygen.

11:24 So, carbon monoxide, combines with oxygen to bond,

11:27 that is by burning in air with a fence blue,

11:31 basically, to form carbon four oxide.

11:34 Like you can see here, okay?

11:35 So, then again, a combination reaction with hemoglobin, okay?

11:41 So, carbon monosa actually combines with hemoglobin,

11:43 which is a HB here, so, in the red blood cells

11:47 to form a carbon dioxide hemoglobin.

11:49 So, it forms carbon dioxide hemoglobin,

11:51 as you can see, this equation here.

11:53 So, basically, this reaction is responsible

11:55 for the poisonous nature of carbon monoxide.

11:59 Basically, as we have the hemoglobin

12:02 be converted to a stable carbon dioxide hemoglobin.

12:07 So, that actually cannot transport oxygen across the body.

12:12 So, in the medical people, of course,

12:14 they have been better positioned to actually

12:17 explain that effect, okay?

12:18 So, now, carbon monoxide also,

12:21 as a reducing agent, it's a strong reducing agent, okay?

12:26 Which actually has the ability to oxidize itself.

12:29 So, basically, as a ability to oxidize

12:32 to cover four oxide in the presence of compounds

12:36 like metallic oxides, basically.

12:39 And steam and iodide also, okay?

12:44 Or iodine oxide.

12:46 Iodine five oxides, you can see here.

12:47 So, it reduces that, because it's a reducing agent,

12:51 it reduces it to CO2, reduces it to CO2 oxide.

12:55 So, as you can see, this PBO,

12:57 then to ease metal.

12:59 So, from this to this metal,

13:01 as you can see, this equation is showing that.

13:04 So, now, it is this thing to hydrogen gas.

13:06 As you can see, this equation here.

13:08 So, it can reduce steam to hydrogen gas

13:10 when you use carbon monoxide.

13:12 Then, also, you have iodine five oxides

13:16 be reduced to iodine, all right?

13:19 So, as you can see, this equation here is showing that.

13:22 Then, basically, uses of CO2 oxide.

13:26 So, we have uses of CO2.

13:27 So, CO2 oxide can be used as fuel by itself, basically.

13:32 So, all in the form of a producer gas.

13:34 So, like, mixture of CO2 monoxide and nitrogen,

13:36 as well as CO2 producer gas, we'll see it as we go on.

13:39 So, also, as water gas.

13:41 So, mixture of carbon monoxide and hydrogen,

13:44 so, CO2 producer gas.

13:45 Don't forget, the first one,

13:46 mixture of carbon monoxide and nitrogen,

13:50 as producer gas, then mixture of carbon monoxide

13:55 and hydrogen is called water gas.

13:57 So, also, it is used as a reducing agent.

14:00 We measure that in the structure of metals.

14:02 This time, for a structure of metals.

14:04 You know, a structure of metals can actually be done

14:07 and done by reduction or by electrolytic method, okay?

14:11 So, we use these carbon monoxide,

14:15 as well as a reducing agent,

14:16 called carrier of that structure of processing metals.

14:20 Okay, so, carbon monoxide can also be used

14:22 in manifold material alcohol.

14:24 So, in manifold material alcohol,

14:26 we can use carbon monoxide.

14:28 So, your form it also.

14:30 So, we can use carbon monoxide.

14:33 You can also use it for gene, for gene.

14:37 Alcohol use for gene also in production of for gene.

14:41 So, we also use that, and so on and so forth.

14:43 So, now, basically, that is for carbon monoxide.

14:47 That's carbon two oxides.

14:48 So, now quickly, we're going to look at carbon four oxides.

14:52 Now, for carbon four oxides,

14:54 now, carbon four oxides is basically

14:56 when carbon two oxides are born in excess oxygen.

15:01 That is when we have carbon four oxides.

15:05 Now, in the bonnie ports,

15:07 basically, we have the top, we have the middle,

15:10 then we have the bottom.

15:11 Now, at the top, we have excess oxygen.

15:13 So, when you bond charcoal, for example,

15:16 you have bonnie charcoal, that is in the bonnie ports,

15:18 for example, all right?

15:19 So, the top is actually carbon four oxides,

15:23 because you have excess oxygen.

15:25 Then in the middle, we have limited oxygen, okay?

15:30 So, carbon two oxides are actually four.

15:32 Then at the bottom, so we have carbon four oxides

15:35 that we produce, because we have excess oxygen

15:37 in the charcoal port, actually, basically, okay?

15:41 So, now, carbon monoxide, and the carbon dioxide

15:44 is one of the two oxides of the elements of carbon,

15:48 and is the main product of carbon form

15:52 from the convoction of hydrocarbon four oxides, okay?

15:55 So, now, carbon dioxide is present

15:58 in the aspirin and is produced by the respiration

16:02 and convoction, all right?

16:04 So, in the aspirin, we can actually produce,

16:07 or have this carbon four oxides

16:09 by respiration, means, and also convoction.

16:13 However, it has a short time in these fields,

16:16 as it's consumed by plants.

16:19 You know, plants consume them in.

16:21 It's just like we breathe in oxygen,

16:24 and breathe out the carbon dioxide.

16:28 Then, the carbon dioxide would breathe out

16:29 is what plant consumes also, all right?

16:32 Just like, because it doesn't actually,

16:34 once it gets into the aspirin,

16:36 it doesn't stay for a long time.

16:37 So, because it's big consumed by plants, also,

16:40 all right, doing photositences, all right?

16:42 So, preparation of carbon dioxide.

16:44 So, carbon dioxide can be prepared,

16:46 just like we have a carbon monoxide

16:49 by heating any metallic carbonate, all right?

16:53 With that looked mineral, that looked mineral axics.

16:57 Of course, you know, mineral axics can be H2SO4,

17:00 can be XCl, can be H2CO3, all right?

17:03 So, basically, like here, the metallic carbonate,

17:07 we use here is calcium carbonate.

17:10 So, it's calcium carbonate here is actually

17:13 be heated with XCl, that they use here.

17:17 You can also use H2SO4.

17:18 Okay, the same result would be obtained.

17:21 Okay, that's what it's for.

17:22 You have calcium chloride, H2O,

17:25 that the most important product here is H2O,

17:28 we are looking for here.

17:30 So, this is actually a diagram showing

17:34 how this thing is done in laboratory.

17:35 So, of course, you have this is,

17:37 all these are the various spec,

17:39 we have the various equipment and the approaches.

17:41 So, like here now, this one is your clump, stand, all right?

17:46 So, this one is TSO4, and of course,

17:47 we should have measured before in your,

17:49 in when I was explaining the laboratory,

17:51 preparation of carbon dioxide.

17:53 Okay, this is TSO4L, of course,

17:55 this one is a kind of round bottom flux, okay?

18:00 Then inside at the bottom of this one bottom flux,

18:04 you have here to be marble chips.

18:06 Now, the marble chips here is actually in the form of,

18:09 your CSU3, okay?

18:11 So, now, what they also added to it was,

18:14 these that looked XCl, the chloric acid, okay?

18:18 So, they are the closer what it does, of course,

18:20 you know that when you drop a castle carbonate in XCl,

18:25 that are the chloric acid now.

18:29 So, the surface area is gonna dissolve faster, all right?

18:32 Because the surface area,

18:33 because it depends on whether it is a lump form

18:36 or it is actually in the powder form.

18:39 So, if it is in the lump form, the surface area is small.

18:41 So, the rate of reaction will be very slow, okay?

18:45 But then it will have fewer amount of product.

18:49 That is the cover for outside.

18:51 Then what the surface area is large,

18:53 then when you, maybe probably you crush it,

18:56 you grind it to make it being in powder form.

19:00 So, the rate of reaction will be faster, all right?

19:03 So, thereby bringing a more amount of product, okay?

19:07 So, this one is just showing us how it is

19:10 the agramatically done.

19:12 So, that's the gadget you are seeing there.

19:14 So, basically, then by heating also, you also use this method,

19:17 by heating it up, or carbonate of metals.

19:21 Carbonate of metal, other than alkaline metals.

19:24 So, like you can use magnesium, you can use calcium here,

19:27 all right? Like here, and then use magnesium.

19:29 These magnesium carbonate will heat it.

19:32 Then it will actually produce a magnesium oxide

19:35 and carbon for oxide.

19:36 This is exactly what we are looking for.

19:37 Then now, also, haven't said these two methods.

19:41 Then, we also look at these properties of carbon for oxide,

19:46 just like we looked at properties of carbon to oxide.

19:50 So, now, first of all, the fiscal properties of carbon for oxide.

19:53 Now, for fiscal properties of carbon for oxide,

19:55 so, now, it is colorless.

19:57 Just like in the first one, it's also colorless.

19:59 This one is also colorless.

20:00 Now, it is soluble in water, of course.

20:02 Now, carbon for oxide is one of the oxides of non-metals

20:07 that are classified under what we call acid and hydrides, okay?

20:11 So, basically, we know that the many points of carbon for oxide

20:16 is minus 78 degrees Celsius.

20:19 All right, that's a multi-point minus 78 degrees Celsius.

20:22 So, basically, then we have the chemical properties.

20:26 Now, you see, carbon for oxide is very reactive.

20:30 Can react with water.

20:31 Can react with metals.

20:33 Can react with muscle carbonates.

20:35 And, you know, you see, the reaction is very vast, basically.

20:40 So, when bubbles into water, so it dissolves slightly

20:44 and some of the carbon monoxide reacts.

20:47 So, forming a solution of weak carbonic acid.

20:50 Of course, this happens when it's raining, okay?

20:54 Basically, when it's raining.

20:55 So, what we have most time is actually the form of acid

20:59 that is formed, there is a weak acid.

21:01 It's all called carbonic acid, basically, okay?

21:04 Which has a pH of five, okay?

21:07 That, this equation is just explaining how this happens, okay?

21:11 So, now, it also supports the convocation of only,

21:16 or strongly, or bunny substances,

21:19 such as, we have it in magnesium, okay?

21:22 So, it supports that also, so magnesium.

21:25 Magnesium method decomposes, all right?

21:29 To, carbon, to, carbon for oxide, basically.

21:33 Like, we showed that in the equation that we have,

21:36 even here, it's also here too, okay?

21:38 So, to provide oxygen for this continued bunny in the gas.

21:43 So, now, here we have this.

21:45 You see, this is a metal here, magnesium metal.

21:48 They react with this to give us this one, and also this.

21:52 So, we actually reduce this carbon to this.

21:55 That's what you are seeing here, okay?

21:56 So, that's what another reaction is actually

22:00 a reduction of oxidation process.

22:03 Now, in that, magnesium is actually oxidizing,

22:06 so, which is the magnesium oxide that we have there,

22:09 then the carbon, carbon dioxide is actually reduced to carbon, okay?

22:13 So, basically, techno.

22:14 So, when carbon dioxide is bubble-true, lime water, and also.

22:18 So, of course, we are going to have the white precipitate,

22:20 which is actually calcium carbonate is formed, okay?

22:24 So, this reaction is actually used as a text

22:28 to actually show that a gas, which is carbon dioxide,

22:32 is present, okay, in a solution.

22:35 Especially when we are carrying out a qualitative analysis,

22:40 that's chemistry practical.

22:41 So, that's the equation that is repeating this explanation, okay?

22:46 Then, now, if carbon dioxide is bubble-true,

22:49 a solution of course is through the solution of continuous sleep.

22:53 So, what happens is that it will eventually become clear,

22:56 not like the other one, maybe probably you bubble just

23:00 limited sort of cloud of it, then, of course, you have some product form

23:07 to some extent, maybe the solution looks so cloudy,

23:10 you know, looks so cloudy.

23:11 You know, when somebody is clouding, it's so clear.

23:14 But, in this case, why you continuously bump lead that?

23:16 This kind of force into the solution becomes so clear, all right?

23:20 Because of the formation of calcium, hydrogen,

23:24 trans-carbonate, all right?

23:26 So, basically, this equation that is explaining this and so on and so forth.

23:31 So, if a carbon dioxide is bubble-true,

23:33 the solution of this, of course, you are going to have a sodium hydrogen

23:37 to carbonate that be precipitated, all right?

23:40 So, there is the equation explaining all that, all right?

23:43 So, use this carbon dioxide.

23:46 So, as a dry accent, we use as dry highs in refrigerators most times, okay?

23:53 So, like, we have in this solid cup of those, as far as I saw, blinds.

23:56 And we also use, as a refrigerant, for high-screen.

24:01 So, also for meat and also for soft food, softened food, also, all right?

24:06 So, it is also used for this purple, because it is colder than highs.

24:13 And it's so blinds, as a melting point, minus 73, I mean 78 degrees Celsius, okay?

24:20 And it does so when it is potentially passed through into a liquid state,

24:28 though it's actually a damaging liquid state, that is, which easily,

24:32 can easily collapse in the process, all right?

24:34 So, that's what that, now it is used in fire extinguisher.

24:38 So, being desan that, that's what we can use it to actually extinguish fire.

24:43 So, in the health, carbon dioxide is actually, which is being evolved from some compounds,

24:50 when due to the preparation of compounds, so it actually helps in reliving in digestion,

24:55 or constipation in medical sector.

24:59 Of course, medical people should be able to explain the use of these to you properly.

25:04 So, now, for fire extinguisher, that's a diagram that is explaining that.

25:07 I'm showing those out, of course, the equipment that can be used for that, for fire extinguishing, all right?

25:13 So, basically, then now, now look at the terms of carbon.

25:16 These are also another form of compounds of carbon now, all right?

25:22 So, don't forget, the topic is others of carbon.

25:25 So, there's also carbonate and hydrogen of carbonate of carbonate.

25:29 So, then the carbonate, basically, and also hydrogen of carbonate.

25:36 So, are inorganic compounds.

25:39 Of course, we know that we actually form numerous compounds with different metals.

25:44 That's probably the most important metals in the electrochemical series.

25:48 So, whenever carbon falls out, it dissolves in water.

25:52 So, of course, we know that it generates hydrogen carbonates, okay?

25:56 So, which is actually a weak, that basic acid, right?

26:00 So, this equation here is trying to just show us how this is done.

26:04 So, basically, this is a ionic form, is weak in that the strength of the acid here,

26:13 because of the presence of this hydrogen at your, is very low, okay?

26:16 So, that's why it's a weak acid here, okay?

26:19 Then now, the acid also reacts by some free metals, example, like zinc, all right?

26:26 Metallic oxide, for example, have a calcium oxide, which is actually a quick line.

26:32 Then we have alkaline's example, we have to do my dosage, all right?

26:36 To form it as a carbonate salt, okay?

26:39 So, metallic carbonates are generally found as natural oils, okay?

26:44 You know, generally, we have all different oils in the form of oxides, oils in the form of carbonates,

26:50 oils in the form of sulfides, sulfides, you know, as so on and so forth, okay?

26:57 So, then this is just a equation showing all that, like we said before.

27:01 Now, the carbonate salt are two types.

27:04 We have the normal transocarbonyl for our salt, then we have the acidic hydrogeyte as a carbonate.

27:10 So, now, basically, in the first one, both of them they have, they have, we have ways of

27:17 preparing them in the laboratory, how we can prepare this in the laboratory.

27:21 Well, basically, for the soluble transocarbonyl, or soluble ones, or soluble salt, so like

27:28 the transocarbonyl now, salt, so the water, the solubility of these transocarbonyls,

27:34 carbonate water, of course, is high, based, of course, we treated that in our previous class,

27:40 where we looked at the solubility of salt in water.

27:43 So, like, for example, we have sodium, we have potassium, we have ammonia.

27:47 These are the most soluble transocarbonyls, right?

27:51 Of which, I know, of which, you know also that the most soluble transocarbonyls are the

27:57 one of potassium, sodium, and ammonia, techniques of that, okay?

28:01 So, now, they are generally made by passic carbonyl oxide, through a solution of corresponding

28:07 alkaline, just like you have it in this equation here, showing you how this happens.

28:12 So, here, we use a general term here, a general symbol here, to show, okay, the various aspects

28:19 of the soluble metals, so like, for example, the every-present sodium, so sorry, we present

28:26 potassium, we present ammonia, ammonia salt.

28:29 So, when all of these variables, now, here, but it's not being represented as, it's somebody

28:35 is represented as an alkaline here, here, sodium, when you put this one here, you have sodium

28:41 hydroxide, then we put this one here, you have potassium hydroxide, then when you put this

28:45 one here, you have ammonia hydroxide, okay?

28:48 So, when they react with carbonyl oxide, so this is what we have, I'll be formed.

28:54 So, this one is a compound of carbon, because carbon is actually found there as an element

28:59 there, all right?

29:00 This is actually M2, M2 here, I show you that, okay, if I put this N here, if I put this

29:08 N here, you have N2 CO3, but put this K here, you have K2 CO3, you have put this one here,

29:14 you have ammonia carbonate, which is NH4, close the bracket to CO3, that's what you have

29:22 here, in this place here, so of course, water is formed alongside with that, so a preparation

29:28 of this soluble one, now the first one we looked at was preparation of soluble one, but this

29:32 is time around, preparation of insoluble, transocarbonyl, so most of the metallic transocarbonyls

29:38 are insoluble, most of them, except the one of what, sodium, potassium, and ammonium

29:44 salt, don't forget that, all right?

29:46 So, the reacts are insoluble, so the common methods for preparing them are very few, though,

29:54 we need to understand this, because if you don't understand how these are, because we use

29:58 this method to select the award preparation, because if you don't understand the method

30:03 which we use in selecting the preparation, so you wouldn't actually know which of these,

30:08 because apart from the three, and make sure, the reacts are, most of them they are insoluble,

30:12 the transocarbonyl form of them, they are insoluble, so reaction, number one, reaction

30:17 of base, with these, with carbohydrates, or basically with most of the trans, so for most

30:24 of the transocarbonyl, with carbohydrates, of course, it will always be, one of the

30:27 bases of, maybe you use a base like calcium hydroxide, you react calcium hydroxide with

30:33 carbohydrates, of course, you put them from a base like carbonate, all right, but it's

30:39 going to be insoluble, so then, now, I don't know, an example, we can also metast

30:44 like zinc, or metallic oxide, example, we have a magnesium oxide, okay, here in this case,

30:51 having the transocarbonyl acid, like this equation is showing us all that, okay, how this

30:57 happens.

30:58 Now, basically, you can also use a method called displacement of transocarbonyl, those

31:05 soluble transocarbonyl, soluble metals, basically like sodium, like atuloportacium,

31:10 or ammonia, okay, the transocarbonyl of them, so like this example is showing you know,

31:16 so the insoluble transocarbonyl precipitated, actually precipitated out, as you can see,

31:22 in this example here, all right, so then, now, the other aspect of the compounds of

31:29 carbon, so the cohydrogen transocarbonyl salts, now, these are actually acidic salts, we know

31:36 that for acidic salt, like we explained previously, in our acid basis, and salt, that when the

31:42 replaceable hydrogen ion is partially replaced by, in meta, so then, we have a pro.co acidic

31:53 salt, all right, so then, again, so for this, we have the soluble one, we have them as

32:01 potassium, sodium, and ammonia, but in this case, the acid salt of transocarbonyl, all right,

32:09 made of whatever in meta, ammonia meta, or radical, all right, so the two, one of the two

32:15 hydrogen atoms in the molecule, so it's partially replaced, don't forget that, all right,

32:20 partially replaced, when it is partially replaced, of course, an acidic salt to be formed,

32:25 so they are actually soluble in water, though the hydrogen transocarbonyl of ammonia, don't

32:31 forget, now the transocarbonyl of ammonia is soluble in water, the transocarbonyl of potassium,

32:41 the transocarbonyl of sodium, they are soluble in water, but in this summer, they are hydro-detrable

32:48 carbonates, they are insoluble, but for other matters, they are also transocarbonyl in

32:57 soluble in water, that's a solid word, this part is showing us here, all right, so and so on,

33:03 and so forth, this is a question of showing that to us, how that happens, so properties

33:06 of transocarbonyl, of course, action of heat, all right, then this is a question of showing

33:11 us how they are heated, all right, so then what happens in the entire hydrogen transocarbonyl,

33:18 as well as decompose on heating, or solid solution to provide carbon-folks, that water

33:24 and the corresponding transocarbonyl, all right, as you can see in this equation, so all

33:28 the transocarbonyl and hydrogen transocarbonyl are reared by dilutes acid to form carbon-folks

33:35 and water, so and also is salt, is formed alongside, so this equation is just showing us how

33:40 that happens, now let's look at some uses of some significant transocarbonyl or salt,

33:48 so for example this is actually used by a manufacturer of glass, so you know, add detergents, okay,

33:54 so then for this one is deployed in baking powder, or to discharge our carbon-folks, right,

34:00 so as that helps to reduce to rice, or throughout the baking process, all right, so then it is

34:07 as well deployed as medicine to relieve the indirection, so we've measured that before,

34:13 so then the castle transocarbonyl is utilized in the production of cement, chalk and significant

34:19 industrial or chemicals, example like castle mugs, like ammonia, you know, and so on and

34:27 so forth, so now basically, I haven't gone through these, you know, lexins, so I believe

34:33 I should be able to evaluate this for me, so what is the density of the amount, basically,

34:39 so which crystals basically crystalline a glass does a graphite actually, a graphite spacing

34:47 may belong, so basically it's actually referring to previous class, all right, so which I was supposed

34:56 to add to the previous class about that, but I did here for you to actually evaluate it also,

35:02 right, so then as soon as so forth, so it's co-considered and allotube, what is the purest form of carbon,

35:10 but basically I would love to ask you my own questions, now the question is that in addition to this,

35:17 are all transocarbonyl soluble in water, that's one, two, are our hydro-t transocarbonyl soluble in water,

35:26 so you'll find out that for me, they then also measure three metals, basically that are very soluble

35:34 in water, in the form of the hydro-t transocarbonyl. Thanks for watching, my name is Charles Christopher,

35:42 till next time.