@@rastiffi Yeah well, he only reads aloud. I would still think that somewhere in between an imaginary god and Professor Dave, there is a good bunch of people who are better at explaing science related material.
You explain in a simple and clear way and in just five minutes. Unlike our professor who spent 1.30 hour to explain it for us.... Ty for your video it really helps me
This was actually fantastic. the first 30 seconds was exactly what I was looking for, and the rest made a lot of sense. Studying for the MCAT and was really confused by this topic!
Dave, I'm doing some passive, elementary studying of chem, and this is the second topic I have been utterly confused from, and only you have concisely explained it enough for this evolved ape to understand.
the particles with greater atomic or molecular size occupy more surface and cause a greater lowering in VP but you say it depends only and only on the number of solutes particles?
I always thought that salt accelerates boiling of water due to it having lesser heat capacity (heard that somewhere). This video made me think and... 1) The supposed change in heat capacity from adding 1 mole of salt to 1 liter of water (55.5 moles) is ~0.5%, with same negliglible heating speedup 2) You'd have to spend extra 1/56 energy on heating salt itself too, so 1.7% slowdown. 3) The boiling point of solution is raised by 0.51 degrees, so another ~1% slowdown assuming water is at 25 degrees initially. So salty will actually boil slower than "pure" water - the tap water already has some dissolved compounds, though.
When he said Let's test comprehension it almost hurt my little pea sized brain. To be more descriptive , it was like watching an air liner fly overhead. But in slow motion. Thanks for the explanation, even if it falls on dead ears.
hey! so I totally understand freezing point depression from the perspective of solutes messing with the crystal lattice structure of solids. but I'm currently studying for the mcat and i was reading online that, above the freezing point, the vapor pressure of a liquid is greater than that of the corresponding solid, and that the opposite is true below the freezing point. and that the vapor pressures of the two phases are equal AT the freezing point. so if we think about it in these terms, if we add solute to a liquid, thereby lowering its vapor pressure, wouldn't that actually raise the freezing point (i.e. make it more "easily freezable")? because wouldnt the vapor pressure of the liquid now be closer to that of the solid? I know this obviously doesnt happen in nature because salt trucks would be causing more problems and not less. but just trying to understand freezing point from the perspective of vapor pressures. thanks!
Sir i have question about this lecture.. sir colligative properties only depends upon the numbers of no volatile solute particles and independent upon the nature of solute nature ... sir if we have two different solutes which have different size of their molecules and larger size molecules solute blocks more particles of the solvent to evaporate hence nature is affected ... can you answer me please sir
i like how random TH-cam are usually much better at explaining than the actually class teacher
He isn't random. He is Professor Dave Explains, second to only god.
@@rastiffi he does resemble Jesus in a way
@@rastiffi Yeah well, he only reads aloud. I would still think that somewhere in between an imaginary god and Professor Dave, there is a good bunch of people who are better at explaing science related material.
@@JaLLaM86 th-cam.com/video/rj4wjFcyaxE/w-d-xo.html
@@rastiffi Thank you for that
You're literally saving lives professor Dave.
Comment still stands 3 years later
@@ssgm1 *4 years later
@@ChristianSolanoP* 5 years later
You explain in a simple and clear way and in just five minutes. Unlike our professor who spent 1.30 hour to explain it for us.... Ty for your video it really helps me
Vapor Pressure and Freezing Point Depression would be some pretty ａｅｓｔｈｅｔｉｃ names for a band, not gonna lie.
My prof took an hour to explain this and I hardly understood it, you took 5 minutes and I instantly understood it. Absolute legend, thank you!
This was actually fantastic. the first 30 seconds was exactly what I was looking for, and the rest made a lot of sense. Studying for the MCAT and was really confused by this topic!
I always dance to the theme song, but then I get serious about chemistry after that.
chemistry dance party!
me tooo hahaha
@@ProfessorDaveExplains what is osmosis and osmotic pressure ?
This is one of colligative properties,isn't it ?
lol same
Hahahha same 😝
Always concise and easy to understand! You're awesome Dave!
Dave, I'm doing some passive, elementary studying of chem, and this is the second topic I have been utterly confused from, and only you have concisely explained it enough for this evolved ape to understand.
You just saved me from 20 pages of crap they have printed in my book!!
Amazing !!
Really easy to understand
NCERT?
12th?
@@notevencalm yeah!
@@abhishekgupte7578 nah mah state board
As a teacher, I consider this video as very informative and clear to understand. Very useful!!
Thanks :)
thanks kindly! please tell your students to subscribe!
Professor Dave Explains I certainly will. Kind regards from Colombia.
These videos are actually great. The pacing makes the content very easy to follow!
Your videos are the best. I dance to your intro and then become serious for studies
professor dave please never change, your videos are so much better than creators like the ochem tutor or tyler dewitt and all them
Thank you for finally explaining Depression in freezing point to me after countless teachers have failed. It finally makes sense now.
I swear u have a power where u can make any complex ideas to explain in the simplest form
Tomorrow is my exam and you are saving me for one more time❤
Professor Dave is better than my chemistry textbook
If only professors taught like you then we would all be geniuses!! Thank you!
I love these lessons. Simple, short, straight to the point.
If I was a teacher I would save trouble by showing those clips to the students; they are exceptional.
Then u should also stop taking salary from the institution, since its professor dave who's doin' ur job . Just kidding!!
you make it short and brief a real definition of professor
I knew it! This guy was the janitor!
This world need more heroes like u Mr.dave
The definition of colligative properties saved my life
Thank you so much! It made my 2-hour learning on this much more clear.
Thanks Prof. Dave! I'm very rusty on 2nd semester Gen chem topics so I'm reviewing to prep before I tutor someone.
sick vid bro, a little something about osmosis would be dope though.
You made things so simple and easy to understand! Thank you a lot, Professor Dave!
Absolutely brilliant . God bless you professor !
Suddenly all my notes makes sense thanks to this video...thank you!!
oh God , YOU ARE AWESOME , so concise yet so AMAZING
Thank you for making my textbook useless hahaha
same XD I haven't used my chem textbook once this year!
@@placid9073 oh hi new comer :D
Really nice video, I am from Ecuador and I am learning English, I like your video
Why tf are we still inflicted with school when TH-cam is a 20x better teacher
Best episode so far!
the particles with greater atomic or molecular size occupy more surface and cause a greater lowering in VP but you say it depends only and only on the number of solutes particles?
Thank you very much sir!!!!
I didn’t understand this topic for a long time, but you explained it so well,ma sha allah.
I always thought that salt accelerates boiling of water due to it having lesser heat capacity (heard that somewhere).
This video made me think and...
1) The supposed change in heat capacity from adding 1 mole of salt to 1 liter of water (55.5 moles) is ~0.5%, with same negliglible heating speedup
2) You'd have to spend extra 1/56 energy on heating salt itself too, so 1.7% slowdown.
3) The boiling point of solution is raised by 0.51 degrees, so another ~1% slowdown assuming water is at 25 degrees initially.
So salty will actually boil slower than "pure" water - the tap water already has some dissolved compounds, though.
You're explaining in a super way sir ,that our mentours can't
When he said Let's test comprehension it almost hurt my little pea sized brain.
To be more descriptive , it was like watching an air liner fly overhead. But in slow motion.
Thanks for the explanation, even if it falls on dead ears.
We all knew the concepts and understand everything, but when it comes to write a PANIC MONSTER enters.
I don't know it's just me , but I love the intro song😂😂😂😂
I'm so thankful for your videos. I'm subscribing right now.
Thank you, chemistry Jesus. You save my test. 🙏
Awesome 👏🏻 vid mr.DAVE
I was once a hater of chemistry but now ....!
thank you so much all the from Brazil!
THANK YOU SO MUCHHHHH!!!!
YOU EXPLAIN SO WELL I APPRECIATE YOU
Sir ur the best saving lives here!
very comprehensive and thorough, good job!
Thank you for the simplified class
All confusions removed !!! Thanks
How about the vant Hoff factor, i?
I ALWAYS make the most stupid mistakes and dont catch them until im looking at the graded test
Thank you prof. Dave 😁 .. this is awesome.
Nice flow Dave
dont you have to account for the particles in the compounds?
Nice video, very helpful. Also osmosis is affected from solute concentration.
exactly what i needed thanks
Thanks professor Dave 👍
This was extremely useful! Thanks professor Dave!
I love Professor Dave's videos!!! He's awesome. He's, he's Beyond Awesome, he's he's BEAWESOME!!!
Also, he looks like Ricky Rubio!!!
Thanks Dave! Your video helped me a lot.
Sir u are a life saver for me..thank u so much sir for such a clean nd neat explanation
Short and sweet.
Thanks
i really didnt think i would understand molality like ever
Professor Dave! Thank you
Beautifully stated.
Saved my life i have an exam tmrw😅
Thank you so much, professor Dave.
I doesn't understand for long time that if solute doesn't vapourised why it make V.P of soln less now Get it up direct to heart ❤️😁
Thank youuu for this wonderful tutorial
sir could you make videos on solubility product..
Thank you Dave!
you explained very clearly thankyou !
my chemistry teacher shared the link of this video in the class
You realize that school sucks when you have to learn through the net just to figure wtf the lesson was about
Thank you professor for shearing with us your knowledge. What are an useful person you are :)
Thank you very much 🙏it is very useful explanation ⚡️
Awesome Professor, thank you! Please smile, chemistry is not that boring. :)
It was explained beautifully by professor dave but unfortunately you left osmotic pressure
Why isn't van't Hoff's factor (i) in those colligative formulas'?
Please make the video on osmosis and osmotic pressure...It is related to solution and colligative property
science made easily understanble
Thank you chemistry Jesus 🙏🙏
Nice!!!you saved my time thanks alot
Thanks professor dave!!!
I'm off to fail my chemistry exam!!!
Dear Dave,Can u make a video on vapour pressure seperately , i wanna know more about how its calculated and the related facts
Why isn't the van 't Hoff factor used in this video?
hey! so I totally understand freezing point depression from the perspective of solutes messing with the crystal lattice structure of solids. but I'm currently studying for the mcat and i was reading online that, above the freezing point, the vapor pressure of a liquid is greater than that of the corresponding solid, and that the opposite is true below the freezing point. and that the vapor pressures of the two phases are equal AT the freezing point. so if we think about it in these terms, if we add solute to a liquid, thereby lowering its vapor pressure, wouldn't that actually raise the freezing point (i.e. make it more "easily freezable")? because wouldnt the vapor pressure of the liquid now be closer to that of the solid? I know this obviously doesnt happen in nature because salt trucks would be causing more problems and not less. but just trying to understand freezing point from the perspective of vapor pressures. thanks!
can you please make soem content on equivalent weight
Very helpful video
THANK YOU FOR THIS SIR!!
Best tutor, thanks sir
Great....... Love you .... Very precise words used
what happened to the freezing of water when salt is added?
Sir i have question about this lecture.. sir colligative properties only depends upon the numbers of no volatile solute particles and independent upon the nature of solute nature ... sir if we have two different solutes which have different size of their molecules and larger size molecules solute blocks more particles of the solvent to evaporate hence nature is affected ... can you answer me please sir
Non-volatile *
Thank you professor dave!!
Do you have a Kb and Kf reference to share, please? I currently cannot find one.
why wasnt the vant hoff factor mentioned?
because glucose is a molecular compound that does not dissociate into any ions as they are not electrolytes. this results in a vant hoff factor of 1