17.4 Solubility and Ksp | General Chemistry

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Thank you very much! While I am quite familiar with the topics explained, my brain tends to be quite scattered and often I get lost in my own calculations or mix-up what I was supposed to be solving for in the first place. Your way of organizing is helping me so much with keeping everything on track.

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My good sir, you deserve all the good things in the world 🙏🏾 explained so so well

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Excellent explanation! 👌Greetings from Belgium🙋‍♂

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[@jimmyhaley6754]

The last part of this video is worth is worth watching the entire video even if someone understands ksp. Tomorrow I have an exam and I know the professor will throw this question at us.

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Thanks for saying so, Jimmy - hope you do well on your exam!

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What the actual fuck??!?? You’re telling me someone who teaches like this acc exist cuz there’s no way i’m acc understanding this concept. Gen Chem final coming up, life saver. Really wish i found this teacher earlier❤❤❤

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Hope you do well on your final.

[@Nomanismyname]

3:02 Why the products' concentration are also x but not x/2?

[@ChadsPrep]

AgCl >> Ag+ + Cl- If you look, the coefficients are all 1 in this reaction, this means that for every AgCl that dissociates, you get an equal number of both Ag+ and Cl- (not half as many each). So if 10 AgCl dissociate, you would get 10 Ag+ and 10 Cl-. Make sense? Hope this helps!

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@@ChadsPrep Yeah,makes sense.Thanks you for your response!

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[@krappy4993]

Idk if you still answer questions on these old videos, Why with Ag2S when we write the ksp equation as Ksp = (2X)²(X) rather (X)²(X)? Shouldnt the stoichometric / molar ratio only appear as a power to X? I get the 2x comes from the change in moles / concentration while ^2 from molar ratio , but the reason you would have 2x is due to said ratio, which is also the case for regular Kc where you only add the ratio as a power... At least thats what i learnt i guess, i assume there are slightly different rules to Ksp than Kc? Thanks for these videos :) i start biochemistry first degrees (bachelor?) in 2 weeks and watching your videos im almost done learning the entirety of general chem planned for this year lol Its truly appreciated that you take your time to functionally teach like half of my degree for free 😅😂

[@ChadsPrep]

Ag2S(s) → 2Ag^+(aq) + S^2-(aq) Based upon the balanced reaction, Now we need to know what to substitute into this expression for the concentrations of Ag^+ and S^2-. Let us suppose that 1 Ag2S dissolved. Then we would get 2 Ag^+ ions and 1 S^2- ion in solution. Let us suppose that 10 Ag2S dissolved. Then we would get 20 Ag^+ ions and 10 S^2- ions in solution. Let us suppose that 50 Ag2S dissolved. Then we would get 100 Ag^+ ions and 50 S^2- ions in solution. Finally, let suppose that we don't know how many (or more properly what concentration) of Ag2S dissolved so we just say that the concentration that dissolves is 'x.' So if 'x' Ag2S dissolved. Then we would get '2x' Ag^+ ions and 'x' S^2- ions in solution. Now we substitute these back into our Ksp expression (which is just a special example of Kc): Ksp = [Ag^+]^2[S^2-] Ksp = (2x)^2(x) Ksp = 4x^3 So the coefficients are used as the exponents in the equilibrium constant expression. But separately, they are the mole ratios (stoichiometry) for the reaction as well. So the coefficients show up in two places after we have substituted the concentrations in terms of 'x,' the molar solubility, back into the equilibrium constant expression. This is a very common point of confusion. Hope this helps!

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[@kathmell]

I'm having trouble solving a problem given to me from class. Is Kc the same as Molar solubility?? Here's the problem given: The molar solubility of Magnesium Phosphate is 5.25 x 10^-6. Determine the concentrations at equilibrium if the initial concentration of the salt in 0.48M.

[@minjinseo3681]

Hello, sir. What will happen to the solubility of BaSO4 if NaCl is being added, and why? Thank you so much.

[@Hellraiser3331]

19 Solubility of barium sulfate in sodium chloride solutions from 25° to 95° Templeton, Charles C. Journal of Chemical and Engineering Data (1960), 5 (), 514-16CODEN: JCEAAX; ISSN:0021-9568. The molal concn. soly. product (K'3) of BaSO4 in the BaSO4-NaCl-H2O system was detd. from 25° to 95° and NaCl molalities of 0.1 to 5.0 as part of a study of scale formation problems from highly concd. brines from oil wells. Ba was detd. spectrographically and total S by a microreduction-colorimetric method. K'3 was found const., within exptl. error, at const. NaCl concn. and const. temp. with varying molalities of Ba++ and SO4--. K'3 increased with increasing NaCl concn. and increasing temp. (K'3)1/2 ranged from 1.08 × 10-5 at 25° to 1.68 × 10-5 at 95° with no NaCl and from 17.7 × 10-5 at 25° to 39.7 × 10-5 at 95° in 5 molal NaCl. Activity coeffs. in the BaSO4-H2O system, calcd. from the Debye-H.ovrddot.uckel limiting law, were used to get activity soly. products (K2). The activity coeffs. were compared graphically with those of ZnSO4, MgSO4, and CaSO4 in the ZnSO4-H2O, MgSO4-H2O, and CaSO4-NaCl-H2) systems, resp.

[@evanr.battallio1115]

isnt it true that Ksp would imply that the reaction is at equilibrium? and if it is at equilibrium that means it is saturated?

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How do you get those zeros ,and x ,x things,am getting the concept but those zeros and x are my barrier

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The playlist covers a standard 2 semesters of undergraduate Organic Chemistry (Organic Chemistry I and II). At my university we also had some advanced organic chemistry courses that were graduate level courses, but this playlist would definitely not be sufficient for those courses. Hope this helps!

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