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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: sci4life on April 04, 2004, 06:32:03 PM

Title: Solubility problem
Post by: sci4life on April 04, 2004, 06:32:03 PM
Suppose that a 10 mL sample of a solution is to be tested for Cl - ion by addition of 1 drop (0.2 mL) of 0.17 M AgNO3. What is the minimum number of grams of Cl - that must be present in order for AgCl(s) to form?

I can't get the right answer...don't know why..please help
Title: Re:Need help with problem
Post by: Mitch on April 04, 2004, 11:04:24 PM
I think you need more information?  ???
Title: Re:Need help with problem
Post by: Donaldson Tan on April 05, 2004, 01:04:25 AM
You need the solubility product constant of Silver Chloride. Only if the product of the concentration of aq Ag+ cation and aq Cl- exceed the solubility product then precipitation of silver chloride will occur.
Title: Re:Need help with problem
Post by: haiph12 on April 06, 2004, 08:42:38 AM
if you get Ksp of AgCl = 1.77×10-10
http://www.ktf-split.hr/periodni/en/abc/kpt.html
then
[Cl-]= Ksp/[Ag+]
[Ag+]=  {0.17*0.2}/10.2
then calculate  [Cl-]  then caculate
mass of Cl-