You have really explain it in a perfect way 😭..especially when you make a difference between saturated and unsaturated solutions....thank u so much 😭🖤✨
The warmer the solvent, the more solute it can dissolve due to the increased motion of the particles. Hotter = faster molecular motion = more frequent collisions between solute and solvent particles). Does that help?
@@infinitasalo472 The heat added enough energy to break the molecular bonds WITHIN solute and solvent, the energy is then released to to recreate new bonds BETWEEN solute and solvent to produce a saturated solution.
If my teacher actually did this it would only take her literally 4 minutes, but I guess she feels since we are in advanced classes we just magically have mastered the art of IPC
+kadiezebra - Give your teacher a break. Recording a 4 minute tutorial takes upwards of 30 minutes (if all goes well and you don't get interrupted) and that doesn't include scripting it out. Not as simple as it looks. Glad you found it useful though!
writing them and again practicing them for days without any idea, rewriting them in the EXAM just to pass, and after the exam we have no idea what we just wrote! Sounds like shit, but it happens! Cant help.......................
Hmmmmm. I think volume has less to do with it than molecular motion. Solubility changes with temperature largely due to increased molecular motion which leads to more “collisions” between solvent and solute particles. As for what role volume plays, I’d have to ask a better chemist! (Great question though!)
Suzanne Tjepkema because the amount of solute that can be dissolved depends on the temperature of the solution. Higher temp = faster molecular motion = more particle collisions = greater solubility. Does that help?
Two things can cause a precipitate to form. In cases like the ones here (where we only have the solution we are starting with, ie. we haven't added any other chemicals to it,) precipitates occur because the solvent can't dissolve any more solute at the temperature and pressure it's at. In the case of MIXING two solutions, a precipitate occurs because a chemical reaction has formed a new INSOLUBLE compound. (That's why the formation of a precipitate is listed as evidence of a chemical reaction. ) Hope that helps!
I can't see the significance of the first step (10c and saturated) in the "supersaturation" part. Why can't we just create a saturated solution at 30c and then cool it down to 10c ?
If you have a supersaturated solution, and you allow some of the solute to re-crystallize, you can physically remove the crystals (aka: chunks). Then you are left with a saturated solution.
Easy! After you've cooled it. Let it sit. If at some point the chunks start to precipitate out it is now a saturated solution (because super saturation requires that the solution continues to hold the solute).
But how can we cool down a solution without getting chunks.??at lower temperature solubility will of course decrease... So chunks must appear... Plz explain
Wait...I dont get it... Does a supersaturated solution really have to be cooled down to be a supersaturated solution? can it be heated? or what if we lower the tempreture of the saturated solution and and adding more solute THEN heat up the Saturated solution, is it still a supersaturated solution? because in our science class, we heated up the mixture... Also....I still dont get it ^^; please someone answer me...This is my homework...
A supersaturated solution is holding (and keeping dissolved) MORE solute than it should be able to at a given temperature. The most common way to achieve this is by making a saturated solution at a given temp and then carefully cooling it. If you heated a saturated solution the amount of solvent would be capable of dissolving MORE solute than it had and the solution would actually be unsaturated. Does that help (or just muddy the water?). Good luck!
Actually, once solute precipitates out of the solution it is simply saturated. A supersaturated solution by definition is HOLDING the extra solute, not allowing it to precipitate.
I know. (My newer tutorials do have better handwriting, this is early work when I was still getting used to writing on the screen). Thanks for watching!
@@ms.heathermoser9104 im really sorry i didnt mean the comment in a derivative way, even though i know it kinda read that way. your vid was very helpful. keep up the good work.
thank you, I have a chemistry test tomorrow. This helped me study.
Snake Breeze good luck
Thank you i have exam tomorrow but i don't understand my teacher so i watched youtube and i can understand this easier
@@rmt6716 yes have good luck on 4 year old comment 🤣😂
Well now it’s 5 🤣😂🤣
@@silveris2cool that reply was 11 months ago
You have really explain it in a perfect way 😭..especially when you make a difference between saturated and unsaturated solutions....thank u so much 😭🖤✨
CORONAVIRUS BRING ME HERE!!!
ANYONE 2020😂😂😂???
Moon Wolf yes helloo
Bruh my chem teacher sent me this and 5 more videos to watch
You really need school you saint bring instead of brought
Yup
Thank youuuu, my chemistry test is only in several hours... you saved me!!
I finally understand the difference between saturated and unsaturated thanks to your tutorial! Thank you so much for the explanation!
thank you i have a science test tomorrow and this really helped me!
This makes SO MUCH MORE SENSE. Thanks Ms.Heather!
Glad it was helpful!
never thought it would be this simple
thanks :)
this helped me study for my chem test thanks so much!!!!!
Honestly. Thank you so much !! Teachers need to be this more understanding. You can't teach " your way ". You have to teach the way people learn.
i loved your short and great explanation. thanks a lot.
Thank you so much...😍😍😍😍🤩🤩🥰 Your teaching capacity is excellent
thanks, it's very simple
Glad it was useful!
Wow.. understand really well now
thank you very much I finally understand this chapter
I’m glad it was helpful!
Thanks helped plenty
Glad I could be helpful!
I thanked you a lot
it helped me...thanks
thank you sm!
Thank you!!!
THANK YOU I FINALLY GET IT!
Yay!
Thank you so much!!!!!!
Glad it was helpful!
Thank you for this great explanation
Good for those who can understand in English
Thank you
Thank you so much. I want to know this so eagerly.
thanks a lot..it really clear my concept :)
thanks
why can more solute be dissolved when the water is heated to 30 degrees Celcius
The warmer the solvent, the more solute it can dissolve due to the increased motion of the particles. Hotter = faster molecular motion = more frequent collisions between solute and solvent particles). Does that help?
@@ms.heathermoser9104 Thanks, that helped me. I had the same question and was scrolling through the comments for help
@@infinitasalo472 The heat added enough energy to break the molecular bonds WITHIN solute and solvent, the energy is then released to to recreate new bonds BETWEEN solute and solvent to produce a saturated solution.
great explanation thanks
Thank you I understanded more
If my teacher actually did this it would only take her literally 4 minutes, but I guess she feels since we are in advanced classes we just magically have mastered the art of IPC
+kadiezebra - Give your teacher a break. Recording a 4 minute tutorial takes upwards of 30 minutes (if all goes well and you don't get interrupted) and that doesn't include scripting it out. Not as simple as it looks. Glad you found it useful though!
If they explained it this way though, it would be so much better than making us write notes that don't make sese
writing them and again practicing them for days without any idea, rewriting them in the EXAM just to pass, and after the exam we have no idea what we just wrote!
Sounds like shit, but it happens! Cant help.......................
Thank you loads!!!!😊😊😊😊 You helped me a lot with my project completion, with this video!!! Thank you!!
Ahana _ Annah_Arrael glad to help!
@@ms.heathermoser9104 ☺️
Great video!
great explanation. Thank you !
Thank you😊❤
Am l right to conclude that the temperature allows for the maximised volume of the solution to dissolve more solute
Hmmmmm. I think volume has less to do with it than molecular motion. Solubility changes with temperature largely due to increased molecular motion which leads to more “collisions” between solvent and solute particles. As for what role volume plays, I’d have to ask a better chemist! (Great question though!)
@@ms.heathermoser9104 Thank you ✨
Why does raising the temperature allow more solutes to be added?
Suzanne Tjepkema because the amount of solute that can be dissolved depends on the temperature of the solution. Higher temp = faster molecular motion = more particle collisions = greater solubility. Does that help?
Thank u so much🖤🖤
Deborah Worku glad you found it useful!
Katie Cook
How do you do solutions? Can you please make a video on it
Do you mean how do you create a solution? Using a solubility table? I could do one of those (but it won't happen soon!). Hope this one was helpful.
Hi i have a question, what factors cause precipitation? does it have to do with the nature of the solution or solute or something else ?
Two things can cause a precipitate to form.
In cases like the ones here (where we only have the solution we are starting with, ie. we haven't added any other chemicals to it,) precipitates occur because the solvent can't dissolve any more solute at the temperature and pressure it's at.
In the case of MIXING two solutions, a precipitate occurs because a chemical reaction has formed a new INSOLUBLE compound. (That's why the formation of a precipitate is listed as evidence of a chemical reaction. )
Hope that helps!
Wait so does the mean that supersaturated solution is only in some cases, like it can’t happen all the time
Thank you for this!
Thank you ❤
Good teaching
Awww! Thanks!
I can't see the significance of the first step (10c and saturated) in the "supersaturation" part. Why can't we just create a saturated solution at 30c and then cool it down to 10c ?
thank u!! It's very helpful!!!
its a good explianation
I don't get it it said that saturated solution cannot dissolve anymore solute and then it said that all solute is dissolved???
Thank you we i more know this for our quiz later
Happy to help!
Nicely Explained... Good Job...
Still have some doubts .... i have sent it though mail so please elaborate me the following..
Thank you.....
What if coffe+water, baking soda+water
I just want to ask, how do you convert a supersaturated solution back to a saturated solution? Please answer thanks
If you have a supersaturated solution, and you allow some of the solute to re-crystallize, you can physically remove the crystals (aka: chunks). Then you are left with a saturated solution.
Easy! After you've cooled it. Let it sit. If at some point the chunks start to precipitate out it is now a saturated solution (because super saturation requires that the solution continues to hold the solute).
For some reason I thought she was going to bust out laughing
thank you, this video helped me a lot!! :)
But how can we cool down a solution without getting chunks.??at lower temperature solubility will of course decrease... So chunks must appear... Plz explain
Ashu Sharma .
Omg thank you so much! This helped so much
very gud and very easy....
tysm i now know their differences
thanks a lot u r a great
DAMN! THANKYOU !!!
Why??
She’s good
Glad it was useful!
Wait...I dont get it...
Does a supersaturated solution really have to be cooled down to be a supersaturated solution? can it be heated? or what if we lower the tempreture of the saturated solution and and adding more solute THEN heat up the Saturated solution, is it still a supersaturated solution?
because in our science class, we heated up the mixture...
Also....I still dont get it ^^;
please someone answer me...This is my homework...
A supersaturated solution is holding (and keeping dissolved) MORE solute than it should be able to at a given temperature. The most common way to achieve this is by making a saturated solution at a given temp and then carefully cooling it. If you heated a saturated solution the amount of solvent would be capable of dissolving MORE solute than it had and the solution would actually be unsaturated. Does that help (or just muddy the water?). Good luck!
Ms. Heather Moser Thank you! ^-^
You didn’t really tell about supersaturation
i still dont get what supersaturated solution is 😭😭😭
A supersaturated solution is holding MORE solute than it should be able to under the conditions of temperature and pressure. Does that help?
@@ms.heathermoser9104 Yes. Thank you very much
thank you very much that was so helpful
god bless you
reemaaz
Wow
Thank you but I still don't understand 😂
me also sister
Haha
SAILOR MOON same don’t know what precipitates mean
hey, just to let you know, supersaturated would make a precipitate. You are wrong dude.
Actually, once solute precipitates out of the solution it is simply saturated. A supersaturated solution by definition is HOLDING the extra solute, not allowing it to precipitate.
had to watch this on my phone bc it wouldnt work on my laptop. my entire class is having this same problem.
Hmmmm. No idea, glad you have the phone!
sa-ta (Sl.) = a kind of local food.
Page 1056
THESAURUS
sate vb 1 = satisfy, indulge to the full, satiate, slake 2 = overfill, cloy, glut, gorge, saturate, sicken, surfeit, weary
If you've ever made a protein shake, you should understand..
guat
PAULINIANS??!!
I had to do this in French like fuck this
lol
You are wrong.
precipate meAN
thanks sexy
You are welcome. Hope it was helpful!
L
you need to work on your hand writing
I know. (My newer tutorials do have better handwriting, this is early work when I was still getting used to writing on the screen). Thanks for watching!
precipite XD
do not try to funny,
Anybody notice that she couldn't spell precipitate
Oops! I never noticed that! I guess I shouldn’t think write and speak at the same time! I hope you still found it helpful.
@@ms.heathermoser9104 im really sorry i didnt mean the comment in a derivative way, even though i know it kinda read that way. your vid was very helpful. keep up the good work.
@@Jakaboyvickery No worries.... I really never noticed, and you are the first person to ever mention it! You should be a proofreader!
Thanks