Precipitation Reactions - Using the Solubility Rules

Basic idea of precipitation reactions. NOTE: when working with precipitation reactions, the solubility rules for ionic compounds are used to determine if a precipitate forms or not.
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[@lucasthethird]

Ben--I have watched about two hours' worth of videos explaining precipitation reactions, aqueous solutions, net ionic equations, and so on. Yours is by far--and I mean by FAR!--the clearest and easiest to understand, with the most well-laid out and clarified examples. Thank you so much!

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Thanks Luke. Means the world to read such a kind comment!

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My left ear really enjoyed this

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lmao relatable (only if u wear headphones)

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its so awkward how much better this guy is than my actual teacher who has way more resources
10/10

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Bless your soul, soooo helpful!!

[@johngraham2186]

Thanks Ben! You're still helping students 9 years later! Very helpful!

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Thank you for your kind words, and thanks for watching! 😀

[@AJay121096]

Thanks so much! I'm having the hardest time in Chemistry, and I've been having to look up a lot of "How to" videos. Thanks for making things simple and easy to understand! :]

[@Finnbrack]

I had no idea how precipitation reactions worked before watching this video, pretty darn confident now, god bless you, sir.

[@anekashah7210]

Thank you so much!!! Had to identify precipitates on my test without even being taught the solubility rules! Looked up a ton of videos and was losing hope until I stumbled across yours. By far, the absolute best!!!! Thanks so much from India!!!

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You're very welcome! Thanks so much for your kind words 😀

[@wholcikedme]

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[@Marcopolo_02]

Its now 2018 and this video has still proven to be useful thanks

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[@tropicallymixed.]

THANK YOU!!!!!!!!!! Anyone reading this, WATCH THIS VIDEO, he explains it well!

[@BensChemVideos]

You're very welcome! Thanks for watching 😀

[@28princesst]

Thanku so much, you make it seem so easy, and yes our teacher is making us memorize that hold chart, along with limiting reactant problems, and finding the emperical formulas from the limiting reactant, and oxidation-reduction rules, not to mention all of the Gas Laws. Some body please pray for me and my classmates!!! But i thankyou for helping me with a clear understanding of precipitaion reactions. Sorry for the paragraph but i had to vent to someone lol

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4 teachers and multiple friends have tried to explain this to me and didn't succeed but in a short 10m you did!

[@misty348]

that was a huge help !!

[@naomibodner8658]

Great video. You made what seemed a very complex part of the chapter very straightforward, easy, and fun. Thank you.

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Thanks a lot, I would say you did better than my teacher that toke two class to explain all of that.

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You're very welcome 😃

[@chipnwafersticks]

Thanks for this. It helped me. I have a reporting in our chem. class tomorrow and I need to discuss this and double displacement reaction. If not for this video, I wouldn't understand precipitation reaction.

[@Rogerrabbit007rb]

Best explanation!

[@alisonhendrix]

Awesome, thanks! Taking chem online and have to learn on my own from the book (tests are done in person on campus but everything else is on our own) and was having a lot of trouble understanding what I was reading. This has helped clear up a lot of my confusion.

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[@TheCrazyStats]

Thank you. I finally understand precipitate much better

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[@LittleMixOf1D]

thank you :) hopefully on the day of my exam(which is tomorrow) I won't forget!!

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+LittleMixOf1D DId you pass lol?

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Thank you. Greatly appreciate the clear explanations and colors. Finally Got!!!

[@Hshidmzajdmz]

Test tomorrow and don't even need to read notes on this..... U explained in 10

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[@hallcory1993]

If you look at the periodic table of the elements, whatever column that the element is in correlates if it is positive or negative.

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[@freepalestine1062]

Thanks man
Great video
Amazing explanation
Examples were very helpful

[@BensChemVideos]

You're very welcome! Thank you for your kind words! 😀

[@freepalestine1062]

@@BensChemVideos wouldn't have said it if I didn't mean it
Seriously helped a lot
Thank you

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thankyou so much.. i actually understand now

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Thanks for the help.

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Thanks for being a cool dude and uploading this.

[@ArtgirlRusher776]

This makes so much sense! Thank you.

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This video is the exact video i am looking for! :D

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Thank a lot ser!

[@wadehamilton5084]

Great video

[@BensChemVideos]

Water is a liquid, so we use (l). Soluble ionic compounds dissociate in water, so we use (aq) for aqueous. Insoluble ionic compounds do not dissociate in water, so we use (s) for solid. Even if an ionic compound is soluble, if it's not in water then it's usually a solid at room temperature, in which case (s) would be appropriate.

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Thank you!! This video helped a lot!

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Lifesaver!

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[@gidielle13]

thanks a lot.. ive seen your other videos and they're really helpful!

[@xkarnx2355]

I wanted to ask from that last question that's Na2SO4 + KCl. When switching how come that so4 doesn't come first and having to determine if it is aqueous or not. Should it be So4K(aq)?

[@perfect204]

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[@abbassyed0]

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[@aru1796]

finally understood something tnx

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[@ALananhR]

Would it be possible for you to do a video(if you have not already) on writing a balanced formula equation, complete ionic equation, and writing a net ionic equation? I am learning it in class, and I am totally and completely lost

[@molly1376]

Why do the pairs switch in the reactions? As in, why are the cations of the reactants paired with the anions they weren't with initially, for the products? Sorry if my question is unclear but this is something I am having trouble understanding.

[@elishasantos582]

Molly Koch Its a chemical reaction called Double Displacement.

[@trayzzay85]

QUESTION!!!!! doesn't the last equation 9:55 have to balance yet? Since it isn't balanced will that affect the outcome? I don't see how it would. IDK

[@elsixters5054]

Great! :)) thanks much.

[@instaminox]

excellent

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Thank you!!!

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THANkS SO MUCH!!!!!

[@ManuelMaciasHouTex]

why did you swap the NO3 and the Br and how do we know whether it is to be swapped or not?

[@nickshep]

Great vid :)

[@RicardoKaka01]

Just a small mistake, for the final equation on 10:27, there should be 2 moles of KCl and 2 moles of NaCl so that it balances out the equation. You need to have 2 K, 2 Cl, and 2 Na on both sides for it to be balanced.

[@bobdan103]

If I pass my chem 103 test today I'm subscribing.

[@johnnyappleseed4020]

thank you!

[@TheQuinnXY]

Wow thx alot

[@mattv11900]

No, because Na is a 1+ charge and there's two of them, and Cl is ALWAYS diatomic (which means it exists in two) and also has a 1+ charge. So Na2Cl2 is just NaCl. :)

[@PurpleEyedPea]

thanks

[@TheMsg911]

Many thanks, my parents included.

[@YoshiHDify]

Is there an easy way to remember the rules. Because in an exam they won't be giving you a clue or any rule sheet. Or do we just have to dead set remember them?

[@parveenshaikh4136]

Why the concentrations of the two solution in a precipitation reactions are different?

[@pauldargan8995]

But the main question that none of these videos address is why the new compounds form - rather than reforming the original compounds? Is it an enthalpic or entropic reason?

[@charlielewis5893]

what if both solutions produced are insoluble?

[@rixon3984]

Then both are precipitates

[@Sarah-ch5vw]

@@rixon3984 I love how you answered despite being 5 yrs late lmao

[@Count_Markus]

good...

[@lovedog49507]

If the compound has a group 1 element is it automatically soluble ?

[@ryanramlogan6512]

In the last example no precipitate was formed but the cations and anions still switched, why is that considered no reaction?

[@elishasantos582]

Ryan Ramlogan I think its not right to say that they dont have reaction. They have reaction but not precipitation reaction because you do not produce a solid precipitate.

[@renee7880]

Sorry, I am new to this. Where did the the 2 go from Na in the last example?

[@Icecube88]

+LZLZLZ ZEE it's because you want it to be in its simplest form. you can reduce Na2Cl2 to NaCl if you divide both by 2. it's in empirical form. I'm guessing you want the compounds in that form when you do this stuff. N2Cl2 is in molecular form.

[@Icecube88]

+Icecube88 yeah, make sure you balance the compounds when you put the elements together. if they can be reduced, then you reduce.
Pb(C2H3O2)2 + Na2SO4 for example. You pair up Pb and SO4. They are balanced, so move on. You pair Na2 and (C2H3O2)2. Acetate (C2H3O2) has a charge of 1-, and there are two of them. Na has a charge of 1+, and there are two of them, so they are balanced. Since they can be simplified though, you simplify them. You can divide both by 2, and that will give you Na(C2H3O2). That's the compound that you will use. So the whole thing together is PbSO4 + Na(C2H3O2). Then you go from there (if they are soluble or not and so on.
Well I want to add that when you do go on from there, you will find that it is a precipitation reaction.

[@Icecube88]

also, you can't reduce polyatomic ions. only if they are in parenthesis (indicating that there are more than one) can you reduce a polyatomic ion..if you get something like Na2SO4 paired up together, then you keep it like that. that's sodium sulfate. sulfate is SO4 with a 2- charge and sodium is Na with a 2+ charge. If you get Na4(SO4)2, then you can reduce it to Na2SO4. notice that the polyatomic ion hasn't changed, so you're good.

[@abdullahsheikh2549]

nice video

[@musketeersmadhouse2262]

Thanks man :-)