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anonymous
 4 years ago
Calculate the solubility of AgCl in a solution containing 0.1M MgCl2 and 0.2M AgNO3
I dont understand why here the reaction moves to reactant
When doing the ICE table, the "C" is x for Ag+ and Cl
anonymous
 4 years ago
Calculate the solubility of AgCl in a solution containing 0.1M MgCl2 and 0.2M AgNO3 I dont understand why here the reaction moves to reactant When doing the ICE table, the "C" is x for Ag+ and Cl

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anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0AgCl> Ag+ + Cl Now There is already Ag+ and Cl in the medium as MgCl2 and AgNo3 are strong electrolytes. Suppose new solubility of AgCl is s AgCl> Ag+ + Cl s+0.2 s+0.2 Ag+ is now s+0.2(0.2 comes from AgNo3) now solve it as (s+0.2)^2=Ksp

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Reaction moves to rectants side according to Le Chateliers principle.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0so do you determine if it moves to reactant side or product side by the Ksp value? I've learnt that Ksp < 0 : moves to reactant Ksp > 0 : moves to product

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0No You are talking about ionic product Ksp is a constant irrespective of the conditions,Anyway if you solve s^2 + Ksp and then find solubility in pure water,you'll find s will be more for pure water than here in this solution. Ksp never changes.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Ksp is always a positive constant.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0but this question given that Ksp AgCl = 1.8 x 10^10 so it is not related on the reaction shifting reactant or to products?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Ksp has nothing to do with it ,it is the solubility s that you should find. Let us take AgCl pure water AgCl> Ag+ + Cl s s s^2=1.8*10^10= approx 1.4*10^5 now lets take AgCl in the given solution. AgCl> Ag+ + Cl s+0.2 s+0.2 (s+0.2)^2=1.8*10^10. Now if you calculate s you get a negative quantity, That basically means the solution is beyond saturated and AgCl starts to precipiate, If AgCl starts to precipitate then reaction is obviously moving to reactants side. I think what you are trying to ask is about ionic product....

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Ionic product= (Ag+)* (Cl) In any sparingly soluble salt if ionic product is greater than Ksp it means that reaction will proceed in backward direction with AgCl precipiating until the concentration of Ag+ and Cl has been reduced till ionic product is equal to Ksp. If ionic priduct is less than Ksp then the reaction will proceed forward with more AgCl disocciating to give Ag+ and Cl Till again the ionic product becomes equal to Ksp.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0i didnt learn about the pure water stuff yet :( and yea, i think i'm talking about the ionic product too my teacher didnt talk much about it we need to find Q and compare it with Ksp if Q is greater than K, then precipitate forms

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0but then since i didnt learn about the pure water stuff, so i cant use ur way to determine if ppt forms or not if i do 1.8 x 10^10 = (0.2 x)^2 x = 0.1999 and 1.8x 10 ^10 = (0.2+x)^2 x=  0.1999 is there another way to detminer if ppt forms other then compare it to water?

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0and thanks for ur help!

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Well the ionic product method is a better method just find the concentrations of the products and multiply them and compare it to Ksp, Finding s is an uneccessary step, I just told you that since you wanted solubility.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0ohhhh i get it now! so 0.2 x 0.2 = 0.04 and is larger than Ksp, that means precipitate forms!! oh thanks thanks thanks!

Preetha
 4 years ago
Best ResponseYou've already chosen the best response.0Great work. Thanks Shanvee for your explanation and thanks LovekBlue for seeking to understand!
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