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Topic: Solubility problem  (Read 5939 times)

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sci4life

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Solubility problem
« 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
« Last Edit: April 24, 2004, 07:06:59 PM by hmx9123 »

Offline Mitch

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Re:Need help with problem
« Reply #1 on: April 04, 2004, 11:04:24 PM »
I think you need more information?  ???
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Offline Donaldson Tan

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Re:Need help with problem
« Reply #2 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.
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haiph12

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Re:Need help with problem
« Reply #3 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-

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