Predicting Precipitation With Ksp Values

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​@@HarshilKapadiya-ii9gp"HE KNOWS ALOT ABOUT SCIENCE STUFF, ITS PROFESSIR DAVE EXPLAINS!"

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[@marianohuelva3029]

precipitation occurs when Q=Ksp or when Q>Ksp cause Q=Ksp refers to a saturated sol'n

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[@MrRandel100]

So, the precipitation will take place when Q is equal to K, or when Q is greater than K?

[@manojmaheshwari4055]

precipitation occurs when Q is greater than K , untill it reaches Q=K.

[@NewWesternFront]

@@manojmaheshwari4055 although precipitation is still happening at q=k, no?

[@waelhawara6251]

@@NewWesternFront same rate for both at that point

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[@davidashiru1842]

Thanks professor

[@halsey2.112]

here's a trick to remember if precipitation occurs when Q is bigger or smaller put Ksp on the left side put a circle then put Q next to it if Q is bigger put < and then draw a line so < and the line represent an arrow now if it points towards reactents it will precipitate like this Ksp

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hi dave , is that playlist complete or are you still adding videos to it ?

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i'll keep adding more over time

[@kagamer21]

Thank you prof!

[@YongeDundasSquared]

i think you used the wrong numbers in the calculations 2.0*10^-4 and you wrote 1.0*10^-4...

[@maceymerdinian3247]

ya, I'm thinking what you're thinking...

[@AllyJaneK]

It's correct. The volume of solution is doubled when mixed, so the concentration is halved.

[@bobwaterson1468]

@@AllyJaneK Is That just for agcl or do you always use half if its synthesis(ex: Ag+Br AgBr) Would the volume be half in this example?

[@sourmango4760]

you are adding 2 solutions of different solutes. They both have equal volume. So the new volume of the mixed solution is double of the separate solutions individually. The amount of each type of salt stays the same but the solution they are in now has double the volume so the concentration becomes half

[@kleeeee]

so like the given values are doubled when mixed, and therefore if i want to get their initial concentration before they are mixed, simply just divide the given into two and will result to 1.0 x 10^-4

[@rassimsimou1594]

Good

[@cyberchampion2675]

Why we subtract from log to get ph

[@lenahalberstadt2587]

In Mn(OH)2 example with minimum pH, how did you get 1.6 x 10^-4M of [OH-]? Aren’t we supposed to divide Ksp (4.5 x 10^-14) by concentration of [Mn2+] (1.8 x 10^-6)? If so, shouldn’t it be 2.5 x 10^-8 and resulting pH 6.4? I can’t figure out where my math is wrong… :(

[@pratikpawar376]

No, because you doesn't taken out of square root of it. Take square root of both side then final answer would be same as it is in video

[@metalrain]

I know it has been a year but why did he square root both sides? How am I supposed to know that?

[@anjalikushwaha8184]

Notice the stoichiometric coefficient on [OH-]² it's squared, that's why...

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YAY I GOT IT!

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Hi professor Dave,you are really amazing professor.I learned lot by watching your Vedio,and I want a go for nursing school for RN in pittsburgh community college,can you please help me for placement test sample questions answer for all subjects I need to get in nursing program.

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Thanks

[@محبيالياسشاكربيلي]

I want an answer to this question👇 The value of Ksp of precipitate in gravimetric analysis should be? a. Very large b. more than one c. non of these d. Very small

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Haircut!!!

[@Damaged262]

Oh come on Prof Dave, who has aqueous solutions of calcium nitrate and sodium carbonate just laying around. Cut the shit.

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thanks