Wish the questions they asked in exams were this easy. You could've increased the difficulty of questions exponentially as you progressed to give examples. Otherwise, really loved the video. Molarity explained in a nutshell. Great work !!
Thank you. You are always make everything easy to be understood. I would like to ask you to explain the idea when we see a percentage in some chemical products. For example 3.5 % Sodium Chloride. Sometimes also we find 99.9% NaCl or 70 % Nitric Acid. So how to make those things related to Molarity. Thank you again
percent is either volume/volume (v/v), which is volume of solvent per volume of solution, or mass/mass (m/m), mass solute per mass of solution, or mass/volume (m/v), mass solute/volume solution. Commercial products often do not say which type of percent they are using. The 3.5% NaCl is likely m/v, so that would be 3.5 g NaCl dissolved in a total volume of 100 mL solution. You can see that this is not a very good measure since 100 mL of solution is not = 100 g, and so the percent does not make 100% sense, but that is very often how it is done. To get molarity you would simply find #mol NaCl in 3.5 g and divide by 0.1 L. The 99.9% NaCl just means there are 0.1% impurities in the preparation. Percent acids are a different story, since it is referring to a percent of the concentrated molar preparation. A concentrated solution of nitric acid is about 16 molar, and so 70% solution is 70% of 16 molar. On the other hand concentrated nitric acid comes out to about 70% m/m, so it may just be referring to that.
Good evening , I’d a question . If I dissolve 5 mole of NaCl in one liter of water, I have a 1M solution : is it correct? But the sum of both volume ( water and salt) is higher than 1Liter. Could you explain me where I mistake?
molarity is moles per liter of solution, not per liter of water. First, you would dissolve the 5 mole NaCl in less than one liter of water, about 800-900 mL because, as you said, the total volume will increase. Once all 5 moles have dissolved, you then add enough water to bring the total solution volume to one liter. You now have 5 moles dissolved per liter of solution. Does that make sense? Second, this would be a 5M solution, not 1M, since you have 5 mole/liter, not 1 mole per liter.
using molarity requires that we have moles, but the problem gives grams, not moles, so the molar mass is used to convert grams to moles. The molar mass (periodic table mass) of NaF is 23.0 + 19.0 = 42.0 g/mol. For NaF, there are 42.0 grams in every mole of NaF, which is what the periodic table masses tell us. Dividing by that converts grams to moles.
@@mohammadwaseemsohail110 You're welcome. You may want to view my video on mole conversions, which gives you a more in depth understanding of molar mass, the periodic table, and mole conversions: ua-cam.com/video/t1pjGbwqt9o/v-deo.html
This is the volume of the solution (as you said), not the solvent. The solution includes all components: the solvent, water, and the solute, NaF. So changing the volume of the solution is irrelevant to the molarity. It stays the same. If you halve the solution, both the amount of solvent AND solute are halved, so the concentration is constant. If you take 1 liter of 1.3 M NaF, half of it, 0.5 L, will have 1.3/2 mol NaF, or 0.65 mol NaF. Hope that makes sense.
There are always some who benefit from disasters. My channel hits have increased quite a bit since lockdown. So while teaching remotely is a drag, I at least get to look forward to seeing how my channel is doing.
In my case i find that teachers make it seems like molarity is different from the concentration A lot of exercices go like this : We have Naoh,10M ........etc calculate the concentration And no its not 10 mol/l
I think they want you to convert molarity to a concentration written as g/l. I remember back in high school they did that and it was confusing. They should just ask "how many grams of NaCl are in 1 liter of 10M NaCl?". Grams/liter or molar, it doesn't matter. Two ways of explaining the same thing. There are some substances where molarity doesn't quite make sense to use , like proteins which are often heterogeneous mixtures of many proteins with different molar masses. Almost nobody would say, I have a 1 molar solution of protein. It'd be mass per volume. mg/ml, ug/ul or g/l
@@ericwright8592 yeah i figured it out at the end i was just in hurry back then ,i had an exam which made me confused glad i got 60.6% in that hell subject ( i have to go through the second exam after 20 days from now though )
After being confused on this for like 2 hours, I now understand it in 5 mins, thank you!
😊
Your graphics make it quick and to the point. Thanks much!
thank you sir this explanation was fantastic, really appreciated.
Thanks, I appreciate your comment.
@@CrashChemistryAcademy no problem sir
I can't thank you enough! Just the way you explained it. Thank you!
I'm glad it helped!
beautifully done. Thanks!
Wish the questions they asked in exams were this easy. You could've increased the difficulty of questions exponentially as you progressed to give examples. Otherwise, really loved the video. Molarity explained in a nutshell. Great work !!
Thanks and an interesting comment. I will put it on my list of videos to do. But it's a long list, so not sure when it will happen.
wow, imagine not understanding this when taught it over 2 days and then watching a 5 1/2 min video and being a pro at it.
¡Qué buen video! Entretenido y al grano. ¡Felicidades!
Muchas gracias, agradezco tu comentario!
Awesome video, this makes much more sense. Thank you so much.
Nice vid! This just help my chem so much!!
You're welcome!
Thank you. You are always make everything easy to be understood. I would like to ask you to explain the idea when we see a percentage in some chemical products. For example 3.5 % Sodium Chloride. Sometimes also we find 99.9% NaCl or 70 % Nitric Acid. So how to make those things related to Molarity. Thank you again
percent is either volume/volume (v/v), which is volume of solvent per volume of solution, or mass/mass (m/m), mass solute per mass of solution, or mass/volume (m/v), mass solute/volume solution. Commercial products often do not say which type of percent they are using. The 3.5% NaCl is likely m/v, so that would be 3.5 g NaCl dissolved in a total volume of 100 mL solution. You can see that this is not a very good measure since 100 mL of solution is not = 100 g, and so the percent does not make 100% sense, but that is very often how it is done. To get molarity you would simply find #mol NaCl in 3.5 g and divide by 0.1 L. The 99.9% NaCl just means there are 0.1% impurities in the preparation. Percent acids are a different story, since it is referring to a percent of the concentrated molar preparation. A concentrated solution of nitric acid is about 16 molar, and so 70% solution is 70% of 16 molar. On the other hand concentrated nitric acid comes out to about 70% m/m, so it may just be referring to that.
Great video! Ready for my Chem exam tmr
Wonderful explanation and your methodology is amazing and works pretty well for me. Thank you very much.🙏
Thanks!🙂
I literally cried for a few days research but finally it is here
quick and clean with no shit talking
Thanks man. I was really struggling in this topic
It is so easy make it heavy unless and other ways continue your teaching
Tnx
u are better than my chem tr
Very informative bro👍
Made easy understanding😊
Makes perfect sense, thanks!!
beautiful! thanks for posting!!
thank you this helped clear things up
What u done u r work on this video amazing for the even don't have aminimum awareness
Thank you so much mannnn
You made my doubt crystal clear ❤
Thanks again ❤❤❤
You're welcome!
Excellent presentation!
awesome Explanation
Understood well. Thanks!
Thank you..was very helpful.
Good evening , I’d a question . If I dissolve 5 mole of NaCl in one liter of water, I have a 1M solution : is it correct? But the sum of both volume ( water and salt) is higher than 1Liter. Could you explain me where I mistake?
molarity is moles per liter of solution, not per liter of water. First, you would dissolve the 5 mole NaCl in less than one liter of water, about 800-900 mL because, as you said, the total volume will increase. Once all 5 moles have dissolved, you then add enough water to bring the total solution volume to one liter. You now have 5 moles dissolved per liter of solution. Does that make sense? Second, this would be a 5M solution, not 1M, since you have 5 mole/liter, not 1 mole per liter.
Crash Chemistry Academy Many thanks
Wow, nice video, I am from Ecuador, I like your video..
Gracias!
Thank You sooooooo Much!!!
Thanks this vedio really I like it👍 😍
danke! Tu bist der beste
Amazing 👌👍🔥
Thanks so much. So easy to understand!! :-)
u earned a sub
Thank you!
Great explanation
Sir can you tell why you divided 42 grams in 2 question please..
using molarity requires that we have moles, but the problem gives grams, not moles, so the molar mass is used to convert grams to moles. The molar mass (periodic table mass) of NaF is 23.0 + 19.0 = 42.0 g/mol. For NaF, there are 42.0 grams in every mole of NaF, which is what the periodic table masses tell us. Dividing by that converts grams to moles.
Thank you very for your wonderful reply
@@mohammadwaseemsohail110 You're welcome. You may want to view my video on mole conversions, which gives you a more in depth understanding of molar mass, the periodic table, and mole conversions: ua-cam.com/video/t1pjGbwqt9o/v-deo.html
nicely done
2:40, wouldn't the molarity be half of .65, not double?
If you increase the volume of the solution wouldn't it make NaF less concentrated?
This is the volume of the solution (as you said), not the solvent. The solution includes all components: the solvent, water, and the solute, NaF. So changing the volume of the solution is irrelevant to the molarity. It stays the same. If you halve the solution, both the amount of solvent AND solute are halved, so the concentration is constant. If you take 1 liter of 1.3 M NaF, half of it, 0.5 L, will have 1.3/2 mol NaF, or 0.65 mol NaF.
Hope that makes sense.
@@CrashChemistryAcademyI think I got it now. Thanks for clearing that up! Means a ton.
You’re welcome! Thanks for watching.
Brilliant
Love from India
Love to India! 💖
Thank you....
You're welcome!
Sir thanks 😄😄
You're welcome!
Can someone explain Me y did we multiply it here 3:45
The question asks for moles but gives liters. The multiplication allows you to cancel liters and end up with moles.
Awesome
Fabulous
Holly shiiit I wish I could give him my tuition, instead of my univeristy of SF!!!
maybe split it?
@@CrashChemistryAcademy I strongly agree that they should split it with you.
Thanks man now ik
Sir 58.5 g is this mass of nacl
58.5 grams per mole is the molar mass of NaCl
Wonderful
Thanks!
2nd question ❓
Best
Who's joe
joe is the molar concentration now take an example we have 25.2 grams and volume 0.75 what is the molarity?
@@lilnugget2280 Joe mama
@@Zak-qp5ln NOOOOOO I HAVE FELL TO THIS TRAP AGAIN
@@lilnugget2280 YOU FOOL
@@Zak-qp5ln NOW IM MAD
How is watching on lockdown 👇
There are always some who benefit from disasters. My channel hits have increased quite a bit since lockdown. So while teaching remotely is a drag, I at least get to look forward to seeing how my channel is doing.
In my case i find that teachers make it seems like molarity is different from the concentration
A lot of exercices go like this :
We have Naoh,10M ........etc calculate the concentration
And no its not 10 mol/l
Not sure what the question would be asking, since 10M is the concentration, or also stated as 10 mol/L, as you said. It is exactly the same.
I think they want you to convert molarity to a concentration written as g/l. I remember back in high school they did that and it was confusing. They should just ask "how many grams of NaCl are in 1 liter of 10M NaCl?". Grams/liter or molar, it doesn't matter. Two ways of explaining the same thing.
There are some substances where molarity doesn't quite make sense to use , like proteins which are often heterogeneous mixtures of many proteins with different molar masses. Almost nobody would say, I have a 1 molar solution of protein. It'd be mass per volume. mg/ml, ug/ul or g/l
@@ericwright8592 yeah i figured it out at the end i was just in hurry back then ,i had an exam which made me confused glad i got 60.6% in that hell subject
( i have to go through the second exam after 20 days from now though )
Reply sir whenever you see my question
First!!!
First