Le Chatelier's Principle Lab with Cobalt Complex Ions

The complete data collection of this classic lab.

[@lj7817]

The music genuinely makes this video unwatchable

[@busdownskipiana2699]

couldnt agree more

[@ninaabregana8281]

I AGREE

[@dawneabdulal-bari9313]

I thought that is was way cool!

[@bananabeast9384]

who else is like a week behind in all their classes for online?

[@hannahl1979]

make that 7 months

[@florianbeyer5748]

@@hannahl1979 hahah

[@xOranfall]

Don’t play music. The music is very distracting.

[@busdownskipiana2699]

very true

[@aradhyavathumilli2193]

Correct

[@maddym7906]

sophomores in chemistry online for quarantine rise up 😔✌️

[@sofiealp3693]

juniors are here too

[@Estoy-127-loco]

and freshmen

[@2time_e939]

yup

[@rstmako]

yall in college? LMAO

[@maddym7906]

@@rstmako highschoolers mate

[@dialecticalveganegoist1721]

You sir, saved me from returning an empty chemistry report! THANK YOU !! Have a nice day!

[@coloraturaElise]

Thanks for a great demonstration! I need virtual labs for my students who are doing testing this time of year, and this is excellent for that purpose!

[@Wargasmo]

This was really helpful, despite the music. Thanks!

[@busdownskipiana2699]

definitely accurate abt the music

[@jameszcurtis]

I agree, the music is too loud and distracting

[@kian4132]

Quarantine Gang

[@2time_e939]

yessir

[@luisiniguez3319]

you sir, are the real mvp -procrastinator in the due date in two hours lol

[@MsDTitmus]

Thanks for posting this! I needed a make-up for my students and the only video I could find showed the Heat in the equations. I also want them to determine the thermochemistry.

[@behnamshamsaddin]

This is an amazing concise representation of Le Chatelier's Principle. Nicely done!

[@ponoanelimpho]

can we chat online i need help

[@zainann8907]

u guys r so mean ! i love the music! better than awkward silence. thank u so much for this

[@chadsartnstuff1143]

i think its just a preference. rather listen to the guy explain what to do than hear the music instead. he could at least turn it down 😂

[@nimalama5504]

Thank you. This was a helpful video.

[@valfinke9801]

very artsy video Grodski !

[@matthewsanders6499]

MAN those poor souls out there with Red/Blue colorblindness are *shook*

[@jaive7]

Crystal clear add blue 😂

[@ScientistRenzo]

Great video

[@ChemTeacher]

Thank you!

[@padik693]

Thanks, so helpful !!!

[@thomasmouratidis8611]

take the music off mate

[@pokleki24]

Amazing video. Thanx

[@MrGrodskiChemistry]

Thanks! You're Welcome!

[@michellequinn7721]

Thank-you!

[@MrGrodskiChemistry]

+Michelle Quinn You're welcome!

[@alexisreyes8006]

Do you think the addition of AgNO will cause a change in the value of equilibrium constant (k) for this reaction?

[@user-jb2ie9fj4l]

Thank you for this video! I am definietly doing this experiment with my class! I do have a question about the hydrated Co complex. Did you buy the Co and then mixed it with water? Or did you buy the cobalt hydrated complex online? Hope you anwser this question!

[@srizz5462]

What a great video . I'm chemistry edu student from Indonesia. Thanks for the explanation sir. I really need this. I'd like to use your video as a reference for my final project. Hope you don't mind about it. Thank you. Best regards ~ Sriza Hayati

[@MrGrodskiChemistry]

Sure! Good luck!

[@jay_snagz]

Turn up the music I can’t hear it loud enough

[@avareinl5448]

What was the chemical name of the precipitate that formed from the double replacement reaction in question 8? And is the heat on the left side of the equation?

[@jamesmckeown8610]

I'm not sure but I think it was silver chloride. The heat is on the left

[@macdaaddyy7505]

what is the role of H and Cl in this lab?

[@juliandavidreyesgalvis550]

Which reacts were used ?

[@orreypadilla3858]

bro the guys phone in the video is ringing and when i hear it i always think its mine ....

[@mindyise]

What if KCl was added instead of HCl? Will the solution turn blue as well? I did this experiment last week, but there wasn't any change in the colour. It only turned blue when heated. Why is it so? :/

[@honourabledoctoredwinmoria3126]

It's the same as with adding CaCl2. It shifts to the blue.

[@colephillips8070]

Saturated KCl solution is only about 4.6 M compared to 12 M HCl. If your solutions are made using water as the solvent the equilibrium will already be shifted far to the left since water is a stronger ligand than cl- A shift right (Blue) will take a lot of cl ions so we need the 12 M HCl. However, if you make the solution with ethanol like in video it will be easier for the cl- ligands to form. So I think KCl would do the trick

[@rachaelmueller4002]

why is that music so loud? it is not the background, its in the foreground,

[@avareinl5448]

How do you tell which way equilibrium shifts? If goes from red to blue is that to the right? And is blue back to light red to the left?

[@MrGrodskiChemistry]

Yes and Yes.

[@user-kg5qi8rh2m]

Let me guess, endothermic right ?

[@dawneabdulal-bari9313]

Cool! Thanks ;->

[@MrGrodskiChemistry]

You're welcome!

[@TheMinionRock]

Hi sir, Could you tell me what was the procedure for handling waste from your solutions? :3 thx in advance; pm i'ts ok

[@shobhadevisingh1106]

Do you by any chance have a list of the materials used in order for me to get the measurements of the chemicals and everything used?

[@MrGrodskiChemistry]

No not really. The solutions are made qualitatively. Also Co in these solutions are a potential exposure hazard .

[@EmanuelePietro]

you could give me your e-mail. I'd like to know which ones are those blue balls that formed after you inserted calcium chloride.

[@mattyoxide3650]

So. Should the equilibrium constant include water in this case? It has an effect if we add more.

[@MrGrodskiChemistry]

You cannot include water in your equilibrium equation that determines the equilibrium constant because water has no molarity or concentration. The law of mass action requires the components of the equation that determine the equilibrium constant have a concentration (molarity of a solution) or partial pressure if the chemicals are in the gas phase. Chemicals that are in the solid phase or liquid phase do not have concentrations while aqueous solutions and gases can. Gases can be considered a solution and can be given a concentration (molarity) as well as a partial pressure. The reason for this is that we track the the equilibrium constant through changes of entropy and solutions can have a change in entropy as they dilute or become more concentrated while liquids (like water) and solids do not.

[@mattyoxide3650]

MrGrodskiChemistry thanks for your reply. I struggle to explain this one. So when adding water is it true to use Le Chateliers principle by saying an increase in the amount of water - not concentration - drives the reaction to the left? Or is it more about the decrease in concentration having a greater effect on the left side thus the shift to the left? That would seem to relate to the equilibrium equation which ignores the water.

[@MrGrodskiChemistry]

@@mattyoxide3650 If you are teaching the concept of Le Chatelier's Principe there is nothing wrong with explaining the increase or decrease of water to drive the reaction BUT the reason that amount water has this effect will require a deeper understanding of equilibrium. As mentioned before, water does not have a molarity but the other components of the chemical equation does. So you are correct in that the water amount will influence the concentration of one of the complex ions more than the other thus driving the reaction. Increasing the amount of water will decreases the concentration of all of the ions on both sides of the equation but the decrease will be less with the cobalt chloride complex on the right side . If you look at the reaction quotient, Q, which has the same equation as the equilibrium constant Keq we will find the answer. The 2 products are on the denominator and one has a power of 4 (Cl-) thus decreasing all the concentrations of all ions the same will cause the denominator to be smaller than the numerator thus increasing the reaction quotient larger than the equilibrium constant (which will only change due to temperature). If the Q is larger than the Keq than the reverse reaction will be more spontaneous and there will be a shift to the left when water is added.

[@Helloworld91976]

would you get the same reaction if you used sodium chloride instead of calcium chloride.

[@MrGrodskiChemistry]

Yes. NaCl has the same common ion as Cl ion in the reaction. It would have the same effect as any chemical species that would provide Cl ions in solution.

[@Helloworld91976]

Okay thank you:)

[@Jaylee0212]

In test tube 3, why does the color change happen when he added silver nitrate?? Can anyone tell me the chemical equation and the reason?

[@MrGrodskiChemistry]

Silver nitrate dissociates into Ag+ and NO3-. Use your solubility rules to see which ion will reaction with available ions in the reaction.

[@Jaylee0212]

@@MrGrodskiChemistry Wow, I didn't expect the answers to come this quick. Thanks for the fast answers and great video by the way

[@MrGrodskiChemistry]

@@Jaylee0212 You're welcome! Good Luck!

[@stacyvaleria2816]

Does anyone know why when he added the silver nitrate it favors the reactants?

[@jrmcr1458]

Por la formación de AgCl(s)

[@colephillips8070]

@@jrmcr1458 I know that is the answer the instructor is looking for but is it also due to the addition of water found in the Silver Nitrate solution? After all the addition of water shifted equilibrium to the pink side

[@wilbertrendonsalvador6524]

o yara mano saludos desde la República Independiente de Arequipa

[@user-mc8vi1vj6n]

can you tell me how you made the mother solution? did you use Ethanol? or NaCl added? what is the concentation of cobalt?

[@MrGrodskiChemistry]

I suggest you stay away from cobalt as it is a possible human carcinogen.

[@user-mc8vi1vj6n]

@@MrGrodskiChemistry thank you for your concern and suggestion. I'm a chemistry teacher in Israel. Cobalt is permitted to use in solutions. of course all necessary cautions will be taken.

[@MrGrodskiChemistry]

@@user-mc8vi1vj6n Please email using link in my channel.

[@lidamagnus6053]

someone help.. why does the AgNo3 cause a left shift? im stuck

[@MrGrodskiChemistry]

Because the Ag+ will combine with the Cl- to form a precipitate (form a solid) thus the Cl- concentration is decreased. The stress of the decreased Cl- ion will cause the reaction to "shift" to the left to increases the Cl- concentration to relive the stress. A precipitate that occurs effectively takes the free chloride ions out of the solution and locks them into the ionic crystal lattice.

[@jameszcurtis]

This helps a lot

[@colephillips8070]

@@MrGrodskiChemistry Is it also due to the presence of water in the AgNO3 solution?

[@MrGrodskiChemistry]

@@colephillips8070 Yes I do think that adding the solution does provide more water which will contribute BUT the precipitate being made is a larger factor in driving reverse reaction.

[@eli.8169]

Any other sophomores in ap chem? I’m so confused

[@bottomtext593]

Visual Learners be like: **Gibberish until you see it unfold before your eyes**

[@user-jt4wn1gf5x]

What is the stress imposed for each?

[@eddiebutkaliuk4681]

Nice try😂😂

[@BingBangBrine]

the music is realy anoying i cant hear

[@ahmaddanish3644]

Can you state the observation of this experiment. Tq

[@quartzlandaker5664]

i think that's your job m8 ;)

[@courtneydodds]

Would you consider the forward reaction exothermic

[@MrGrodskiChemistry]

Students are using this lab as an assignment and I would rather not that answer that directly. The answer to that question is presented with the observation in the cold/hot water test. If you know whether an exothermic or endothermic reaction is favored when heated or cooled, you have the answer.

[@busdownskipiana2699]

@courtneydodds its endothermic

[@brianechipare8157]

@@busdownskipiana2699 thanks my guy

[@aydenrooklidge2095]

bus down skipiana thanks bro

[@EmanuelePietro]

can you write me the chemical reaction between the pink cobalt chloride and the calcium chloride ??

[@MrGrodskiChemistry]

Well the reaction is the one written above the demonstration. The reaction shifts or becomes more spontaneous in one direction as you add this salt. I do not want to totally explain this here as students are using this video for lab. Please email me and I will explain further if you desire.

[@kiramariano7530]

is the forward reaction endothermic or exothermic

[@MrGrodskiChemistry]

Use your observations in the last to tests in this video to answer this question.

[@jacoposiena8028]

@@MrGrodskiChemistry mokka a mammt

[@ArjanD78]

Nice demonstration! The music is SUPER distracting though

[@MrGrodskiChemistry]

Yes I should have done without it

[@aydenrooklidge2095]

THE FORWARD REACTION IS ENDOTHERMIC I THINK

[@cozysundae]

Could you tell me how much the [Co(H2O)6]2+ solution or the mixing methods of [Co(H2O)6]2+ ? Pls I need to do this experiment. ㅠㅠ

[@MrGrodskiChemistry]

The preparation of the complexes is purely qualitative however I would advise against this preparation due to the toxicity and hazards that Co presents.

[@williamfitzgerald2419]

What was the concentration of the concentrated HCl used?

[@MrGrodskiChemistry]

It was concentrated HCl. When I did this in class I dispensed the acid for the students.

[@williamfitzgerald2419]

My teacher says he has 12 M but it is too dangerous for a student to use.

[@MrGrodskiChemistry]

Agreed, hence the video.

[@williamfitzgerald2419]

Right, so if I wanted to do this, could I dilute the HCl?

[@getsemanirios4967]

@@MrGrodskiChemistry whats Is the product of HCl + CoCl2?? Help me pls

[@zaraamjad7151]

why is everybody hating on the music?

[@zaraamjad7151]

#bepositive

[@mursyidmuhajir1502]

Heellooo..... It's me

[@yogaharyutama6395]

I know thank you

[@mynanic]

music giving me ptsd

[@antiplayz2915]

Music drive me crazy had to exit and watch another video

[@Pllm30]

that background music....

[@alyssamichaelaflores1708]

Is the reaction as written endothermic, or exothermic? Justify your answer.

[@nostalgic6876]

bruhhh this assignment makin us do multiple choices for reasoning and evidence. screw this.

[@DEVIL-005]

Try posting without music

[@jayrextong4674]

hi bs chemistry STUDENTS HAHAHAHA. LAST LAB REPORT. FIGHTINGGGG!! :D

[@dontfollowmethanks6980]

Who was your teacher lol

[@maecabalcar3978]

Music is okay, if u want to learn the CONTENT, focus only to it...not on the music.

[@paytonarriola7803]

music way too loud g

[@MrGrodskiChemistry]

Yeah I have learned from all these comments that I should forget the music.

[@NewWesternFront]

mr. flying V shredding for his life was a little out of place when trying to analyze a chemical reaction

[@user-jb2ie9fj4l]

Hello! I would like to ask you a couple questions about the concentration of the cobalt complex, Could I have your email ? To ask yu some questions?

[@lorenzero]

7:28

[@christophergibbons3631]

please no music with your videos. it is a little difficult to concentrate.

[@MrGrodskiChemistry]

You have the ability to turn the audio off as it is a virtual lab.

[@thatguygaming6798]

who’s here from miss browns class

[@febha_mathew]

music is not the right vibe my guy.

[@elnoraibragimova7301]

please off your music

[@ClearSummerSkies]

Great video, but that music has got to go.

[@JHVermaat]

CO = carbonmonoxide; cobalt = Co

[@MrGrodskiChemistry]

Absolutely correct. Thanks for the edit. That mistake is made in my metal ion complex diagrams BUT not in the reaction used in the virtual lab.

[@KeepMyHerringbone]

Helloooo

[@sachaweisz2108]

turn off that music

[@aidanbertone1840]

Bruh Ap chem as a junior Dont do it its a trap

[@leogonzalez2087]

100 pesos al que me lo traduzca al español

[@OmarMora]

I HATE IT HERE 😐

[@arale6460]

please do not ever make a video with music like this ever again

[@davidenander823]

bad

[@lissa_bea]

juniors in chem online for quarantine STILL check in ✌️🤡