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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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! :]

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

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Thank you. I finally understand precipitate much better

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

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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.

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THANK YOU SIRRR !

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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 😀

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

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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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[@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)?

[@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

[@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.

[@ManuelMaciasHouTex]

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

[@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

[@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.

[@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?

[@lovedog49507]

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

[@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.

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[@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. :)

[@parveenshaikh4136]

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