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Need help calculating solubility, please?
Please help with this problem. I'm not sure where to begin.
The solubility of pure lead chloride is 4.41g/L=.01586mol/L. I calculated the Ksp of lead chloride to be 1.595x10^-5. What is the solubility of lead chloride (PbCl2) when disolved in .1M NaCl solution?
Thank you.
1 Answer
- ?Lv 48 years agoFavorite Answer
The solubility of NaCl should be known before making any other calculations. I posted a page from wikipedia saying the solubility of NaCl in water is 359g/L = 6.14276mol/L; this means the .1M NaCl will dissolve completely. The important piece to look at is the Cl- ions because PbCl2 and NaCl have the chloride ions. An ICE Table should be constructed to find the solubility of PbCl2.
PbCl2 -> Pb2+ + 2Cl-
I - 0 0.1
C - +x +2x
E - x 0.1+2x
Ksp = (x)(0.1+2x)^2 = 1.595*10^-5
x = 0.00150mol/L = solubility of lead chloride when dissolved in .1M NaCl solution.
Source(s): http://en.wikipedia.org/wiki/Sodium_chloride