January 15, 2025, 12:44:45 PM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Common Ion Effect and HCl  (Read 3112 times)

0 Members and 1 Guest are viewing this topic.

Offline nonlinear

  • Regular Member
  • ***
  • Posts: 27
  • Mole Snacks: +0/-0
Common Ion Effect and HCl
« on: February 27, 2010, 08:19:59 PM »
Hi, I have a question about the common ion effect.
In general, if I dissolved AgCl2 in a strong acid, it wouldn't make a difference in its solubility, correct? HCl is a strong acid so the Cl- ions would not have any significant affinity for the H+.
My question is this: What if AgCl2 were put into a solution of HCl? HCl would fully dissociate, so there would be an initial concentration of Cl- in the solution. Wouldn't that decrease AgCl2's solubility in HCl (aq)?
I want to know if my thinking is correct, that's all. Thank you!
Logged

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27897
  • Mole Snacks: +1816/-412
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Common Ion Effect and HCl
« Reply #1 on: February 27, 2010, 08:44:02 PM »
What is AgCl2?

You are right about strong acid not making any difference. You are also right about presence of chlorides lowring solubility of silver chloride.
Logged
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Offline nonlinear

  • Regular Member
  • ***
  • Posts: 27
  • Mole Snacks: +0/-0
Re: Common Ion Effect and HCl
« Reply #2 on: February 27, 2010, 09:03:30 PM »
Oh! sorry, AgCl. I don't know what I was thinking.
Alright, thanks!
Logged
Pages: [1]   Go Up
« previous next »
Sponsored Links