I appreciate these videos. You do a great job introducing chemistry and science concepts. I use them all the time for summary in my NGSS STEM Chem class. Thanks!
At first I didn't understand how to use the common ion effect quanititatively, so I paused the video as soon as you said "quantitative," went away for two days, and came back knowing how to do it using the Ksp expression (without having finished the video until today, which confirmed my hypothesis). It's amazing how much we integrate and learn in diffuse mode.
This was the last topic on my exam syllabus and after finishing the rest of the syllabus I still couldn’t understand the concept and that’s when I found this video. Thanks a lot Professor Dave
Wow !!!! Thank you so very kind. I was missing out one point ending up getting wrong values as I failed to understand when studying alone using Zumdah Zumdah..... expecting more from you Professor Dave
Common ion effect is an application of Le Chateliers Principle. If we were to add one component the equilibrium will shift to one side and add to that side. Two compounds sharing the same ion adding them to a reaction will promote precipitation.
Hello professor Dave! I bring you mind boggling chemistry question if it is ur willing Let me explain the question and i want satisfactory and simple tangible answer Q: In Our chemistry lesson i.e "Acid-Base equilibria" we have learned about acid-base conjugate with their strength (based on Bronsted-Lowery acid base pair) so #1👉)if HA (Hypothetical Acid) is weak, it's conjugate base will be stronger than it's source acid i.e HA, again #2👉 if HB (hypothetical base) is weak, it's conjugate acid will be much stronger than HB. #3👉 if HA is strong, the conjugate base will be weak #4👉 if HB is strong, it's conjugate acid will be weak #5👉 also Ka & Kb are directly proportional to the strength of acid and base (i.e when the value of Ka & Kb increase acid and base strength also increase ) Based on this as we know NH₃ is weak base and it's conjugate acid must be stronger and must contains higher Kb value. However NH₃ which has Kb value 1.8×10¯⁵ i.e higher than it's conjugate acid i.e ka value of 0.556×10¯⁹. so even if we use big approximation we get the ff 🔵Kb=10⁴ka according to the above definition the value of NH₄ (conjugate acid) must be much larger than it's source base. Why is this so? according to the above 5 definition doesn't it contradicte? as i mentioned i need deep clear and convince answer rely on book (also you have to make a video on this topic )
1:15 why do we add potassium iodide we could have applied a different iodide compound not specifically potassium iodide and 2:06 where did cadmium bromide come from. 3:29, why do we have to root the value 1*10^-28
1:45 the addition of KI increases I- concentration, so the reaction shifts left. Why doesn’t the K+ in KI affect the shift? Is it because it doesn’t react with anything on either side?
Does the molar solubility of AgI and KI decrease, or does the solubility of AgI decrease and the solubility of KI increase? Is it possible for KI to precipitate out when its added to a solution of AgI? I think the slightly less soluble salt precipitates first but if the saturation point of the solution is exceeded then both salts form precipitate.
The 0.010 M Cd2+ ions were present due to CdBr2. But, there were no S2- ions. When you add CdS, it dissociates into Cd2+ and S2-. Since equal number of both ions are released in this process, we add X to both the concentrations
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Anyone else having there chemistry exam tomorrow....
Yes
Me😭😭😭
Today 🥺😭😭
In 3 hours actually 😭
Yes
Once upon a time I knew this.
Why learning again ?
Damn
Got carried away by the new look 😂❤
rightttt... the first thing i noticed😂😂
I clicked because of the haircut!!!! #clickbait 🤣
Same here. Shock!
Same
Me too
+1
common hair effect .d
Wow you got a new haircut, looks good! Funny how hair can make people look so different.
absolutely right 😂
I appreciate these videos. You do a great job introducing chemistry and science concepts. I use them all the time for summary in my NGSS STEM Chem class. Thanks!
Yes... Ions are easy when the handsome profesor Dave explains..
thx a lot, i don't understand this concept in class but you use 4 minutes to explain this so clearly.
Hi Professor Dave! I love your videos and also your haircut XD, you just earned a new sub!
Damn, Professor Dave. Lookin' good
At first I didn't understand how to use the common ion effect quanititatively, so I paused the video as soon as you said "quantitative," went away for two days, and came back knowing how to do it using the Ksp expression (without having finished the video until today, which confirmed my hypothesis). It's amazing how much we integrate and learn in diffuse mode.
Except I forget to come back to where I paused lolol
This was the last topic on my exam syllabus and after finishing the rest of the syllabus I still couldn’t understand the concept and that’s when I found this video. Thanks a lot Professor Dave
Wow !!!! Thank you so very kind. I was missing out one point ending up getting wrong values as I failed to understand when studying alone using Zumdah Zumdah..... expecting more from you Professor Dave
omg first time seeing professor dave like this
Thank you sir frm bottom of my heart .short video but great Explaination..your leacture is really fruitful for me .love frm Pakistan ♥️♥️
paper ke tayari ho gaye😂😂😂
Y'ALL sleeping on my boy Dave...he always hit different 😘
Nice haircut! Thank you for helping me to pass organic chemistry. Great video too, Professor Dave
Holy crap. You look better brother. Keep this
Common ion effect is an application of Le Chateliers Principle. If we were to add one component the equilibrium will shift to one side and add to that side. Two compounds sharing the same ion adding them to a reaction will promote precipitation.
what is the difference between Le Chateliers Principle and Common ion effect. i am japanese
his haircut got me simpin over Prof Dave 🥺
THE HAIRCUT!!!!! PROFESSOR DAVE HAD HIS HAIR CUT!!!!!
Thank you for uploading beautiful explained videos
And I loved your new hair cut
I use to watch ur videos all the time it's very helpful...by the way nice haircut 💯
Ur channel is saving me for mcat
i am literally stunned at how you made it look so simple.....YOU ARE AN ALIEN....Amazing video...i used to criticize you...more love to you!!!
your videos are super concise and epic
Nice Brother .
Thanks Dave I learned a good amount from your videos
Hi Professor Dave!
Final is tmmr, this is helping a lot lol
Practical me kaam ayega aaj tgank u sir ❤️
Great video dude!
RUclips just recomended this to me and its 275 views
I guess youtube knows i love science
You will get many more of his videos in you recommendations.
Great job man!!! Keep up the good work!!!
L comment
Hello professor Dave!
I bring you mind boggling chemistry question if it is ur willing
Let me explain the question and i want satisfactory and simple tangible answer
Q: In Our chemistry lesson i.e "Acid-Base equilibria" we have learned about acid-base conjugate with their strength (based on Bronsted-Lowery acid base pair)
so
#1👉)if HA (Hypothetical Acid) is weak, it's conjugate base will be stronger than it's source acid i.e HA, again
#2👉 if HB (hypothetical base) is weak, it's conjugate acid will be much stronger than HB.
#3👉 if HA is strong, the conjugate base will be weak
#4👉 if HB is strong, it's conjugate acid will be weak
#5👉 also Ka & Kb are directly proportional to the strength of acid and base (i.e when the value of Ka & Kb increase acid and base strength also increase )
Based on this as we know NH₃ is weak base and it's conjugate acid must be stronger and must contains higher Kb value. However
NH₃ which has Kb value 1.8×10¯⁵ i.e higher than it's conjugate acid i.e ka value of 0.556×10¯⁹. so even if we use big approximation we get the ff
🔵Kb=10⁴ka
according to the above definition the value of NH₄ (conjugate acid) must be much larger than it's source base.
Why is this so? according to the above 5 definition doesn't it contradicte?
as i mentioned i need deep clear and convince answer rely on book (also you have to make a video on this topic )
You should start an MCAT series!!
I plan to do that at some point!
was awesome
understood very well
thank you so much
Thank you soooo much savior.
Thank you professor! the new haircut looks great by the way
brochago your the man
This was very helpful :)
That's great man
thank you
Thank you sir ..nice explanation 🙏🙏🙏
Thank you!
Really love u r videos keep it up Were supporting u :)
Thanks professor dave :)
I was shocked by the new haircut.😅❤
In the ksp expression, why haven't we divided it by concentration of CdS
Because CdS is in the form of precipitate (solid) and the active mass of solid is 1. So we don't include that while writing the ksp expression.
determine the ph of 1.0 M KF. the value of hf is 7.2 × 10−4
DOPE hair cut ! i missed your long hair
Thanks bro
New lesson
New haircut
🖒
Don't believe him.. He isn't professor Dave.. He's one of his clones 😂😂😂
But I think Ksp value doesn't change(does change if only temperature is changed). Kip value increases to equilibria the formula
Thank you sir
explain diverse ion effect too
ty chemistry jesus
Nice Haircut :)
Professor Dave hits different every time
your dumb
1:15 why do we add potassium iodide we could have applied a different iodide compound not specifically potassium iodide and 2:06 where did cadmium bromide come from. 3:29, why do we have to root the value 1*10^-28
I thought Professor Dave got replaced
Clear.
The worst part of the MCAT? Having to relearn Gen Chem stuff you thought you were done with :(
1:45 the addition of KI increases I- concentration, so the reaction shifts left. Why doesn’t the K+ in KI affect the shift? Is it because it doesn’t react with anything on either side?
yes potassium is inert in this case
hmmm
I have my paper today
More on electro chem😊
New haircut, same chemistry Jesus
NOOOOOO THAT BEAUTIFUL HAIRRRRR
Does the molar solubility of AgI and KI decrease, or does the solubility of AgI decrease and the solubility of KI increase? Is it possible for KI to precipitate out when its added to a solution of AgI? I think the slightly less soluble salt precipitates first but if the saturation point of the solution is exceeded then both salts form precipitate.
Sir why did we added 0.010+x anf not 0.010-x as the molarity will decrease on use?
The 0.010 M Cd2+ ions were present due to CdBr2. But, there were no S2- ions.
When you add CdS, it dissociates into Cd2+ and S2-. Since equal number of both ions are released in this process, we add X to both the concentrations
Oh, wow! What a handsome guy :) looks nice
Wow ! Nice haircut ! Sir!😆
YES! Did you get a haircut or is it hiding
Student: Professor Dave!
PD: Yes
Student: Why do you look like Adam Sandler with a Beard?
PD: The Common Ion Effect
anyone here in 2024
Present
i dont understand where the 0.10 from the cadmium bromide came from
wow bro nice haircut!
nice
you really dialed in your green screen holy shit
Woww u got a hair cut
Nice
Finally decided to get a haircut, looks much better
You look like ranbir kapoor of Bollywood
He looksss diffrenttt
###thnx sir###
i STILL DON'T GET IT UGH
I miss your long hair chemistry jesus
I didn't really understand
It! Wish you
had gone deeper to make it clear for beginners too
should watch the other vid, like i the earlier ones, he uploaded them too
Cute head
Rip
💜💜💜💜💜
Why did you cut your hair?
Hey man you are more handsome after your haircut
I came here because of the haircut, not because of chemistry hahaha lol jk
Nooo his hair 😞
who dis man
اول عربيه😂❤
NOOO his hair is gon ;-;
Nice haircut
I will miss your hair