Strong Electrolytes include: strong acids, strong bases, very soluble compounds. Weak Electrolytes include: An insoluble ionic compound, weak acid, weak base You have to have all the acids and the solubility rules memorized if you guys are confused as to wtf is going on.
1. you have to memories strong acids and then every other one is just weak 2. all salts are going to be strong electrolytes regardless of solubility and strong acids all also be a strong electrolyte
FYI this video is great for practice. I would look up and memorize what are you strong bases, acids, and soluble/insoluble salts first. Then use this as practice. If you come here without even trying, it could probably not be the best. But if you come to this video prepared, it feels like such a great boost!
This is so frustrating! How do we know what compounds are strong/weak acids/bases? Is that just memorization? If so, why doesn't any video just let us know?! I get that electrolytes and strength/weakness have a direct relationship, but how do you determine that?
Hello, I hope this helps There are really only 7 strong acids so most people memorize them: HCl: Hydrochloric acid HNO3: Nitric acid H2SO4: Sulfuric acid HBr: Hydrobromic acid HI: Hydroiodic acid HClO4: Perchloric acid HClO3: Chloric acid The most common strong bases are metal hydroxides that come from the first two columns or periods of the periodic table. Example: NaOH and LiOH are strong bases. (If your teacher is picky there are also things called super bases but I am going to assume they are out of the discussion for simplicity) Salts are also strong electrolytes (see a definition of salt from a chemistry perspective) Most people assume that if it is an acid and it is not one of the strong ones then it must then be a weak acid and the same is true for bases.
I know this has been like 3 years ago, but if anyone is needing help with this, you are needed to be able to remember that non electrolytes are covalent compounds, or a non metal and non metal, such as glucose. However, some like NH3 does have covalent compounds and the nitrogen is extremely soluble in water, making it a weak base. Strong acids would have a H+ in front, with them constituting to the saying of CSI NBC, or Charlie Brown Is Now Super Charles, and weak acids would be the opposite of these 7. Stronger bases would start with a group 1/2 ion combined usually with a hydroxide.
@@or638 yes that should be right. As well as yeast would consist of all covalent compounds, remember that yeast could be used to make bread by dissolving in sugar water.
After practising for months now i'm starting to get a good idea of what constitutes a strong electrolyte.. but a lot of it is memorization. This is important stuff to know about for questions involving the common ion effect/ LCP, etc
Professor Organic Chemistry Tutor, thank you for a short and sweet explanation of How to Identify Weak Electrolytes, Strong Electrolytes and Nonelectrolytes in AP/General Chemistry. The strong/weak acids and bases increases my understanding of this material. This is an error free video/lecture on RUclips TV with the Organic Chemistry Tutor.
This video was so helpful!! I was originally confused as to why HF wasn't a non-electrolyte being that it is, in theory, a covalent compound (nonmetal + nonmetal). Most covalent compounds are non-electrolytes. However, because this video pointed out that it is a weak electrolyte, it made me remember Fajan's rule--- that HF has more ionic properties than covalent due to differences in orbital size. So because HF has ionic properties, one can consider it an electrolyte. But since HF isn't soluble in water, due to the solubility rules, it won't be a strong electrolyte.
Okay- This is a late post, but a great breakdown. Solubility is not equal to electrolytes. Solubility is determined by the solubility charts. Strong electrolytes are Ionic Compounds or Molecular Compounds that semi-ionize (7 Strong Acids/8 Strong Bases) Weak Electrolytes tend to be anything that ionizes just a tad (Weak Acids/Weak Bases) Non-electrolytes are usually molecular compounds.
thank u so much. i had dowloaded tons of ur video pls keep it up. you are great teacher! i'm migrating from non science to science pls always make it easier ans simple for someone like me. thanks alot u have been a great help.
Well, I noticed most of strong electrolytes are either strong acid or strong basic as well as salt from strong acid and strong basic. But, NH4Cl which is salt from weak basic and strong acid is strong electrolyte? How do you determine if the solution is strong or weak? Is NH4Cl the exception?
This is what I think, correct me if wrong: NH4Cl is considered an ionic salt due to the NH4+ (cation) and Cl- (anion). Due to the soluabity rules, it disassociates completely making it a strong electrolytes as the water molecules surround the respective free flowing ions which now allow it to conduct energy. It’s not considered an acid + base, don’t let that confuse you. Just a polyatomic cation + anion.
Basically electrolytes include strong acids, strong bases, and highly soluble salts. Weak electrolytes include, weak acids, weak bases, and slightly soluble salts. According to the solubility list NH4Cl is a highly soluble salt and as an ionic compound so it does act as a strong electrolyte
Sigma rule : any compounds which contains no3,so4,cl they are strong electrolyte rest of them are weak electrolyte💫 you can easily solve any type of question 😉 #neetaspirants
@@breannabuiYes you’re right because salts that generally contain Cl- are soluble, but if a halide salt like Ag+ Pb2+ or (Hg2)2+ then it would make it insoluble. Hence why AgCl is insoluble.
A common misconception is that insoluble ionic compounds are weak electrolytes. In fact all ionic compounds are strong electrolytes, because that which is dissolved exist entirely as ions in water. Even insoluble ionic compounds (e.g., AgCl, PbSO4, CaCO3) are strong electrolytes, because the small amounts that do dissolve in water do so principally as ions; i.e., there is virtually no undissociated form of the compound in solution. That which is insoluble exists in the solid crystal phase and is therefore by definition not in solution and even "insoluble" ionic compounds have some degree of solubility however small. The extent to which an electrolyte dissolves in solution does not indicate whether it is strong or weak. It is the relative proportion of dissociated and associated species in solution. For any ionic compound, all of the species in solution are dissociated.
Hey man. Usually your videos are great, but this one didn;t explain how to know if each compound is ionic or molecular which determines their ability to conduct electricity lol.
But why though, I already have lists of strong/weak acids/bases. How do you determine which is more or less soluble. My solubility chart looks just like everyone else's just soluble/insoluble?
I don’t know what ur soluble chart is but basically: 1- sodium, potassium, and ammonium r soluble 2-chlorides are soluble except when they’re with Agcl, Hgcl, Pbcl2 however pbcl2 is soluble in hot water and Hgcl2is soluble. 3- sulfates are soluble except with Strontium, calcium, mercury, barium and lead. 4- phosphates, silicates, and carbonates are insoluble except with Sodium, potassium and Ammonium. 5- Sulfides are insoluble except with Calcium, strontium, potassium, sodium, and ammonium. Hope this helped
Sadekin Khan it’s completely soluble because while hydroxides are insoluble, they have the exception of Barium (Ba).I’m sure you knew that, but the exception means that it is completely soluble, not just slightly!
Ba(OH)2 is a strong base thus it acts as a strong electrolyte, u shouldn’t be confusing solubility with electrolytes, only take solubility rules when working with salts.
i had searched for is sucrose (genshin impact character) weak or strong and u know what!!! this video poped up😅, i think i got the answer and that is Sucrose is strong as HCl😂
Dissolving is when a compound breaks apart into isolated particles. The second process is when a substance dissociates. Dissociation is when an ionic compound dissolves and breaks apart into constituent ions.
AgCl is a strong electrolyte, solubility and electrolyte strength are unrelated. While it is true that electrolytes are caused by ions in a solution, solubility is a relative term. Everything will dissolve but some to a far lesser extent. Because of this all salts are strong electrolytes. This is as there will still form Ag+ and Cl- and we measure electrolytes based of the ions formed. Thus is a strong electrolyte even though it does not break up completely.
@@raghur561 Aren F is correct. Although AgCl has very low solubility, a simpler way to put it is whatever amount of AgCl dissolves, however little, completely breaks up. In other words, there are no AgCl molecules floating around in the water as a single entity, because all of them have dissociated. This is obviously very late but I hope this clarifies any doubt you have not clarified by now.
You have to memorize the schedule of acids and bases, strong acids, strong bases and highly soluble salts are all electrolytes. However, weak acids weak bases and slightly soluble salts are all weak electrolytes.
idk if you need this anymore but if a compound has a high solubility it also ionises more in water (generally). Therefore it will be a stronger electrolytes as the ions carry the charge
Confused as to why HF and NH4Cl are in different categories. Both NH4 and HF are weak acids and both are also soluble in water. So why is one a strong electrolyte and the other a weak electrolyte?
HF is a weak acid that partially dissociates into H+ and F-. about 90 to 95% will remain undissociated as HF in water making it a weak electrolyte. NH4Cl is a strong electrolyte because it dissociates completely (nearly 100%) into NH4+ and Cl-. The NH4+ ion is a weak acid that further dissociates into NH3 and H+ but only to a small extent like HF. less than 10% of the original NH4+ will convert into NH3 and H+. NH4Cl is both a highly soluble ionic compound and a weak acid. HF is not ionic but is a weak acid. The ionic features of NH4Cl explains why it's a strong electrolyte and why HF is not.
there is a mistake in this video slightly salt should be a strong electrolyte. because even if the small amount of salt when reacting in water it produces ions. Solubility is not mean ionization so, most of the salt even if sparingly salts are strong electrolytes
ruclips.net/video/hxNoZ9ZYt7k/видео.htmlsi=CTvjEGVfAhS7LZc8 go to this guys youtube way more in depth and will actually help you determine how to know if it is a strong electrolyte weak electrolyte or non electrolyte
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Strong Electrolytes include: strong acids, strong bases, very soluble compounds.
Weak Electrolytes include: An insoluble ionic compound, weak acid, weak base
You have to have all the acids and the solubility rules memorized if you guys are confused as to wtf is going on.
Bruh you just saved my chem grade
@@shouryaseth5715 lol
straight up ur better than my chem teacher
NaCl is ionic compound , so it's weak electrolyte according to your comment 🙂.
@@NaifIT11 NaCl is very soluble, so it's actually a strong electrolyte according to the comment
Things to search first before watching this:
1. How to know if they're weak / strong acid
2. How to know if they ionize in water
thanks!
Couldn't figure things out until I searched up both of those things. After that this video was great practice.
1. you have to memories strong acids and then every other one is just weak
2. all salts are going to be strong electrolytes regardless of solubility and strong acids all also be a strong electrolyte
@@oodsdonk2423 Mg(OH)2 is a weak electrolyte though?
@@oodsdonk2423 only soluble salts are electrolytes
FYI this video is great for practice. I would look up and memorize what are you strong bases, acids, and soluble/insoluble salts first. Then use this as practice. If you come here without even trying, it could probably not be the best. But if you come to this video prepared, it feels like such a great boost!
Where are you from l am from India
Seriously 🙏🙏🙏🙏🙏
This is so frustrating! How do we know what compounds are strong/weak acids/bases? Is that just memorization? If so, why doesn't any video just let us know?! I get that electrolytes and strength/weakness have a direct relationship, but how do you determine that?
right ive been trying to figure this out too.
Do a quick search on strong and weak acids/bases. Yes, its pretty much memorization but there's mnemonics to help like BICPENS (strong acids)
No, you cant memorize all of them. Memorize solubility rules.
Cynthia Sabazali organic chem explains some of it due to resonance in understanding weak/strong acid/bases
Hello, I hope this helps
There are really only 7 strong acids so most people memorize them:
HCl: Hydrochloric acid
HNO3: Nitric acid
H2SO4: Sulfuric acid
HBr: Hydrobromic acid
HI: Hydroiodic acid
HClO4: Perchloric acid
HClO3: Chloric acid
The most common strong bases are metal hydroxides that come from the first two columns or periods of the periodic table. Example: NaOH and LiOH are strong bases. (If your teacher is picky there are also things called super bases but I am going to assume they are out of the discussion for simplicity)
Salts are also strong electrolytes (see a definition of salt from a chemistry perspective)
Most people assume that if it is an acid and it is not one of the strong ones then it must then be a weak acid and the same is true for bases.
I know this has been like 3 years ago, but if anyone is needing help with this, you are needed to be able to remember that non electrolytes are covalent compounds, or a non metal and non metal, such as glucose. However, some like NH3 does have covalent compounds and the nitrogen is extremely soluble in water, making it a weak base. Strong acids would have a H+ in front, with them constituting to the saying of CSI NBC, or Charlie Brown Is Now Super Charles, and weak acids would be the opposite of these 7. Stronger bases would start with a group 1/2 ion combined usually with a hydroxide.
Well written
@@or638 yes that should be right. As well as yeast would consist of all covalent compounds, remember that yeast could be used to make bread by dissolving in sugar water.
@@or638 haha I wish I could help! I'm only a High Schooler. It sounds very interesting
your voice is so relaxing. chemistry is my favorite class but is often stressful. your videos before bed are so nice
thank you
Tosh kurdy 7iz al
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My teacher keeps referring back to your channel as supplemental material. I love how you making things easier to understand the main point
This video increased my confusion 🤣🤣😅
It's true 🤧
Like a seriously
No, it only shows how good your teacher is, I completely understood everything because my teacher has taught me well about it.
After practising for months now i'm starting to get a good idea of what constitutes a strong electrolyte.. but a lot of it is memorization. This is important stuff to know about for questions involving the common ion effect/ LCP, etc
Professor Organic Chemistry Tutor, thank you for a short and sweet explanation of How to Identify Weak Electrolytes, Strong Electrolytes and Nonelectrolytes in AP/General Chemistry. The strong/weak acids and bases increases my understanding of this material. This is an error free video/lecture on RUclips TV with the Organic Chemistry Tutor.
How can you tell if the ionize ?
Or tell if they are an electrolyte
This video was so helpful!! I was originally confused as to why HF wasn't a non-electrolyte being that it is, in theory, a covalent compound (nonmetal + nonmetal). Most covalent compounds are non-electrolytes.
However, because this video pointed out that it is a weak electrolyte, it made me remember Fajan's rule--- that HF has more ionic properties than covalent due to differences in orbital size.
So because HF has ionic properties, one can consider it an electrolyte.
But since HF isn't soluble in water, due to the solubility rules, it won't be a strong electrolyte.
Okay- This is a late post, but a great breakdown.
Solubility is not equal to electrolytes.
Solubility is determined by the solubility charts.
Strong electrolytes are Ionic Compounds or Molecular Compounds that semi-ionize (7 Strong Acids/8 Strong Bases)
Weak Electrolytes tend to be anything that ionizes just a tad (Weak Acids/Weak Bases)
Non-electrolytes are usually molecular compounds.
Your videos are pulling my grades up omg!!!!!!!
3 years later your still helping me
You’ve helped me a lot, thank
thank u so much. i had dowloaded tons of ur video pls keep it up. you are great teacher! i'm migrating from non science to science pls always make it easier ans simple for someone like me. thanks alot u have been a great help.
Well, I noticed most of strong electrolytes are either strong acid or strong basic as well as salt from strong acid and strong basic. But, NH4Cl which is salt from weak basic and strong acid is strong electrolyte? How do you determine if the solution is strong or weak? Is NH4Cl the exception?
This is what I think, correct me if wrong: NH4Cl is considered an ionic salt due to the NH4+ (cation) and Cl- (anion). Due to the soluabity rules, it disassociates completely making it a strong electrolytes as the water molecules surround the respective free flowing ions which now allow it to conduct energy. It’s not considered an acid + base, don’t let that confuse you. Just a polyatomic cation + anion.
Basically electrolytes include strong acids, strong bases, and highly soluble salts. Weak electrolytes include, weak acids, weak bases, and slightly soluble salts. According to the solubility list NH4Cl is a highly soluble salt and as an ionic compound so it does act as a strong electrolyte
@@selamkirby1401 all salts r ionic salts, as salts r formed from cation from a base and and anion from an acid.
Sigma rule : any compounds which contains no3,so4,cl they are strong electrolyte rest of them are weak electrolyte💫 you can easily solve any type of question 😉 #neetaspirants
Agcl is weak though....
@@Rivi.i i think Cl is strong unless paired with a hard metal? (just speculating, not entirely sure. someone please fact cjeck me.)
@@breannabuiYes you’re right because salts that generally contain Cl- are soluble, but if a halide salt like Ag+ Pb2+ or (Hg2)2+ then it would make it insoluble. Hence why AgCl is insoluble.
A common misconception is that insoluble ionic compounds are weak electrolytes. In fact all ionic compounds are strong electrolytes, because that which is dissolved exist entirely as ions in water. Even insoluble ionic compounds (e.g., AgCl, PbSO4, CaCO3) are strong electrolytes, because the small amounts that do dissolve in water do so principally as ions; i.e., there is virtually no undissociated form of the compound in solution. That which is insoluble exists in the solid crystal phase and is therefore by definition not in solution and even "insoluble" ionic compounds have some degree of solubility however small. The extent to which an electrolyte dissolves in solution does not indicate whether it is strong or weak. It is the relative proportion of dissociated and associated species in solution. For any ionic compound, all of the species in solution are dissociated.
first time watched ur video.
Teaching very well. but ur teaching vry fast.
He’s much better than this. This is just a practice mostly
So if you had like MgBr2 would that be strong electrolyte or a weak one?
I honestly dont know whats going on in chemistry lmao
Hey man. Usually your videos are great, but this one didn;t explain how to know if each compound is ionic or molecular which determines their ability to conduct electricity lol.
Sorry it has been 2 years, but basically, strong acids weak acids and weak bases are molecular compounds. Strong bases are ionic compounds.
Good work God bless you 🤗
But why though, I already have lists of strong/weak acids/bases. How do you determine which is more or less soluble. My solubility chart looks just like everyone else's just soluble/insoluble?
I don’t know what ur soluble chart is but basically:
1- sodium, potassium, and ammonium r soluble
2-chlorides are soluble except when they’re with Agcl, Hgcl, Pbcl2 however pbcl2 is soluble in hot water and Hgcl2is soluble.
3- sulfates are soluble except with Strontium, calcium, mercury, barium and lead.
4- phosphates, silicates, and carbonates are insoluble except with Sodium, potassium and Ammonium.
5- Sulfides are insoluble except with Calcium, strontium, potassium, sodium, and ammonium.
Hope this helped
Your videos are sooooo helpful, you explain way better then my teacher, and your voice is so calming
How df do you know which compound ionizes and which doesn't?
CaT V you practically have to memorize them
you need to know the difference between ionic and covalent bonds first.
then solubility rules, strong and weak acids.
I found this video so helpful 50 mins before my exam 😅😅😅
Your videos have saved my grades! Thank you and stay awesome 😎
Hello There is a problem solving of electrolytes and nonelectrolytes..??
Thank you very much!!
Which software you use for lecture video , tell please
What is the difference between ionization and hydrolosis
According to solubility rules., Ba(OH)2 is slightly soluble. Therefore, it should be a weak electrolyte. Or am I missing something?
Sadekin Khan it’s completely soluble because while hydroxides are insoluble, they have the exception of Barium (Ba).I’m sure you knew that, but the exception means that it is completely soluble, not just slightly!
Ba(OH)2 is a strong base thus it acts as a strong electrolyte, u shouldn’t be confusing solubility with electrolytes, only take solubility rules when working with salts.
Can you do one for conductivity in solutions...
Very helpful!!!
So how are we supposed to know if it is a strong are weak acid?
Memorize the schedule
i had searched for is sucrose (genshin impact character) weak or strong and u know what!!! this video poped up😅, i think i got the answer and that is Sucrose is strong as HCl😂
god i love his voice
😭
Can anyone pls tell me how ammonium acetate is a strong electrolyte
Thanks. It very helpful.
can u explain WHY its a strong weak or nonelectrolyte? ...not just say the answer -.-
Completely dissociate, incomplete dissociate, and no dissociation
Dissolving is when a compound breaks apart into isolated particles. The second process is when a substance dissociates. Dissociation is when an ionic compound dissolves and breaks apart into constituent ions.
You’re better then my teacher
Which organic compound is a strong electrolyte??
None of organic compounds are strong, take formic and acetic acid as an example.
AgCl is a strong electrolyte, solubility and electrolyte strength are unrelated. While it is true that electrolytes are caused by ions in a solution, solubility is a relative term. Everything will dissolve but some to a far lesser extent. Because of this all salts are strong electrolytes. This is as there will still form Ag+ and Cl- and we measure electrolytes based of the ions formed. Thus is a strong electrolyte even though it does not break up completely.
Aren F this is not right
@@raghur561 Aren F is correct. Although AgCl has very low solubility, a simpler way to put it is whatever amount of AgCl dissolves, however little, completely breaks up. In other words, there are no AgCl molecules floating around in the water as a single entity, because all of them have dissociated. This is obviously very late but I hope this clarifies any doubt you have not clarified by now.
I have a question that asks which substance is an electrolyte and 3 of the choices are all based and acids idk which one to pick
You have to memorize the schedule of acids and bases, strong acids, strong bases and highly soluble salts are all electrolytes. However, weak acids weak bases and slightly soluble salts are all weak electrolytes.
So i need to memorize if that's a strong acid or nah?i don't get it how could you identify it just by looking at the compound
Doesn't explain exactly how we can identify them or do we have to memorize it all?
Taiwo shogbanmu you have to memorize it all, this video is for someone who has memorized them and now needs practicing
Not really I didn’t memorize them just the rules. Because there are way more that no video can cover
What is the relationship between solubility and electrolytes?
idk if you need this anymore but if a compound has a high solubility it also ionises more in water (generally). Therefore it will be a stronger electrolytes as the ions carry the charge
SIR, IS CH3COONa a strong electrolyte ?
im pretty sure it aint
Nope most organic compounds are weak electrolytes
Confused as to why HF and NH4Cl are in different categories. Both NH4 and HF are weak acids and both are also soluble in water. So why is one a strong electrolyte and the other a weak electrolyte?
HF is a weak acid that partially dissociates into H+ and F-. about 90 to 95% will remain undissociated as HF in water making it a weak electrolyte. NH4Cl is a strong electrolyte because it dissociates completely (nearly 100%) into NH4+ and Cl-. The NH4+ ion is a weak acid that further dissociates into NH3 and H+ but only to a small extent like HF. less than 10% of the original NH4+ will convert into NH3 and H+. NH4Cl is both a highly soluble ionic compound and a weak acid. HF is not ionic but is a weak acid. The ionic features of NH4Cl explains why it's a strong electrolyte and why HF is not.
My professor also includes insoluble ionic compounds under non-electrolytes. Confusing.
He said that Ethanol is polar but in reality Ethanol is non-polar
Thanks bro!
So basically double check on the solubility table..?
there is a mistake in this video slightly salt should be a strong electrolyte. because even if the small amount of salt when reacting in water it produces ions. Solubility is not mean ionization so, most of the salt even if sparingly salts are strong electrolytes
What markes acetic acid a Weak electrolyte?
Thank you!
Thank you.
Wow brief explanation thanks 😍
You are great
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This makes so much sense! Thank you
This title is misleading.
great thank you
THANKS
Where are you from
Aare sir ji jara acche se boliye aap indai me rehte hai😊
so many thx
How the heck do we know if it’s an acid or not? Your not explaining anything.
+2/2 INT
Do work sir!
ruclips.net/video/hxNoZ9ZYt7k/видео.htmlsi=CTvjEGVfAhS7LZc8
go to this guys youtube way more in depth and will actually help you determine how to know if it is a strong electrolyte weak electrolyte or non electrolyte
Okay but how?
These videos are boring but useful
nice
Agcl is strong electrolyte,
Agcl is a strong Electrolyte OKKKKKKKKKKK
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