Solubility and the Born-Haber Cycle
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- Опубликовано: 6 сен 2024
- Why do some things dissolve in water while others don't? Is a supersaturated solution just a beaker with a cape? Let's talk about solubility, the Born-Haber cycle, and more!
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Congratulations on becoming the first person to have explained the born-haber cycle to me!
thank you chemistry Jesus
Does anyone know *1)* why raising the temperature normally increases solubility (making the said supersaturated solutions) *2)* and why for the Ce2(SO4)3 it is the opposite see min 1:15 ? BTW thank you, Prof Dave!! I'm trying to go thu the entire playlist, not only for chem and it has been of great help!
well two reasons, more heat means more kinetic energy, but also things that are entropically favorable such as dissolution become more spontaneous at higher temperatures due to the gibbs free energy equation
U and @theorganicchemistrytutor are my actual lectures
Ong
these videos are really clearing things up for my chem final thank you
Katherine Gilmore same here
4:13 isn't it Cl- ?
oh man! that's a pretty dumb error. thanks for catching that!
Thank you Professor Dave for your awesome videos. In this video, I know you set aside entropy to simplify the explanation. However, did you notice that the enthalpy does not favor dissolving of these salts? They are all endothermic. We need an entropy increase to make this happen. What do you say?
Why would it be favorable to dissolve if the hydration energy is GREATER than the lattice energy? Don't atoms want to be in the lowest energetic state?
well it's kind of like more energy storage gets the system to a lower energy. can get confusing, i know.
I thought that when atoms bonded, they will have a lower overall energy. How do these concepts compare or link together? Thank you for replying, Professor Dave! Your videos are very helpful :)
it's true, the system will go to a lower energy, though i like to refer to it as "energy storage", since it will require energy to disrupt the bonds. in the end as long as the numbers are working out the language is secondary!
You are right! This video has mistake: solubility is thermodynamically favourable because of entropy. Enthalpy can't explain why NaCl is soluble in water. But the author didn't not tell anything about it.
@@AntonAleksashkin entropy is introduced later in the series. and no, enthalpy is also involved in dissolution if the ion-dipole interactions produced outweigh the lattice energy. spontaneity depends on both enthalpy and entropy.
does water get colder when you dissolve salt into it or does it get warmer? and what is this hydration energy? does the hydration energy (if you were to add it to the part of the lattice structure with sodium and chlorine ions) basically lower the energetic state of the thing below the NaCl solid?
the only way i can make sense of the salt dissolving into the water is if the energetic state of the solution is lower than the solid state, so the water would get heated due to some energy release. i couldnt find anything googling for it though
Hydration energy is the enthalpy change on hydrating a mole of anhydrous salt. Since NaCl dissociation is endothermic, it should raise its own enthalpy, thus lowering the solvent temperature. Although I didn't fully understand the portion after parentheses, I'll just say that hydration energy lowers the energy of the lattice, since it is inversely proportional.
Disclaimer: I'm still in grade school, so what I've written is solely based on what I've been taught. If I was redundant or wrong anywhere, please do correct me...
Underrated prof. Dave ep
U just earned a new subscriber ❤
Best explaination ever !
Short nd to the point.
Sir in magnitude is lattice enthalpy is same as enthalpy of formation
More organic chemistry, please
+kevjtnbtmglr coming soon!
Deadpool: I am marvel jesus
Professor Dave: Well, I am chemistry jesus.
Helpful video😁understood it easily
sir u are to good thank you its nice from learning u
why half of cl2?
Really man you are so good.By the way are u really a professor and at where you are working as professor? just curiosity not to hurt your feelings. thanks
+Asshwin M not teaching too much these days, focusing on curriculum development and science communication, mainly looking to expand this channel quite a bit. look out for new content soon, and tell your classmates!
Thank you
Excellent video
Good
Why is solubility dependent on temperature? Once a solute has used up the ion pairs that can be formed with the solvent, a higher temperature will not create more solvent ions to pair with, or does it? It sounds like you are saying a higher temp. creates more solvent molecules than existed at a lower temp.
so don't forget that higher temperatures means greater kinetic energy. if you have a solid sitting in solvent, the faster the solvent particles are moving, the more capable they will be of breaking apart the interactions of the solid. also higher temperatures mean more vibrational energy for the solute particles, making them more likely to dissolve. thermal expansion of the solvent is also a factor!
Where do you get the kJ numbers? Do they need to be memorized from a certain table?
Great explanation by the way!! :)
you don't need to memorize! it's all tabulated data you can just refer to at any time.
Jesus, this was really helpful!
Why do you never use Caps?
i like to shorten things to phrases with as few words as possible and if it's not a complete sentence i prefer to not capitalize. just an aesthetic choice!
3:15 born Haber
im prepping for jee and watching this lol
3:45 why is -355 not -246
it's the electron affinity of chlorine
Jesus? is that you? been three days since I last saw you. Gott Sei Dank
davisha
Do you have an unbuttoned collar to let it breathe? Because you gotta let that shit breathe bro.
+Zglorxk for sure, bro. letting that shit breathe, bro.