Equilibrio of a sparingly soluble ionic compound

  • Chemistry
  • Thread starter daphnelee-mh
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  • #1
Homework Statement:
Calculate the concentration of the first cation until second cation just starts to precipitate as sulfate
Relevant Equations:
Ksp
I got the first question correct but I don’t understand the answer given for second question which is c (Pb^2+) = 8.4x10^-5 molL ^-1. It divided the concentrate for sulphate ion of Ag2SO4 into 2 , but it is the solubility right ?
7D54C1EC-7177-41A4-A391-D1ADE92A3573.jpeg
 

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Answers and Replies

  • #2
Borek
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This is very difficult to read :mad:

It divided the concentrate for sulphate ion of Ag2SO4 into 2

As far as I can tell - it didn't.
 
  • #3
1577086669679.png

My answer is 4.33 x 10^-5, but answer given is 8.4x10^-5, how can I get it?
 
  • #4
Borek
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Next time please type the answer (takes less time than writing and taking pictures).

As far as I can tell answer given is wrong, your approach looks OK.
 
  • #5
Sorry, my computer have problems that time, I can just upload using phone. Therefore, is it the given answer is wrong?
 
  • #6
Borek
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Looks like, I got the same answer you did.
 
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  • #7
chemisttree
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Were you given the Ksp for PbSO4?
Wikipedia has it at 2.13X10^-8 (20C), the CRC has it at 1.06X10^-8 (18C) and you are using 1.3X10^-8!
 

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