December 23, 2024, 08:06:45 AM
Forum Rules: Read This Before Posting


Topic: Le Chatelier's principle  (Read 2966 times)

0 Members and 1 Guest are viewing this topic.

Offline hopeful

  • Regular Member
  • ***
  • Posts: 9
  • Mole Snacks: +0/-0
Le Chatelier's principle
« on: November 01, 2006, 08:20:34 PM »
I am just learning of Le Chatelier's principle and was wondering if this reation that I thought would work.

NaCl(s)-->Na+(aq)+Cl-(aq)

(Note: enough NaCl would be dissolved for the water to be completely saturated)

Now if I was to add HCl (which dissociates to H+Cl-) to the right side would solid NaCl form in the bottom of the container (due to le chatelier's), or what would exactly happen seeing as once the HCl is added you now have a stress of Cl- in the system?

Thank you

Offline Donaldson Tan

  • Editor, New Asia Republic
  • Retired Staff
  • Sr. Member
  • *
  • Posts: 3177
  • Mole Snacks: +261/-13
  • Gender: Male
    • New Asia Republic
Re: Le Chatelier's principle
« Reply #1 on: November 01, 2006, 09:03:28 PM »
NaCl(s)-->Na+(aq)+Cl-(aq)

Your chemical equation isn't entirely valid.

In a saturated solution,
NaCl(s) <-> Na+(aq)+Cl-(aq)

Now if I was to add HCl (which dissociates to H+Cl-) to the right side would solid NaCl form in the bottom of the container (due to le chatelier's)

Yes, you are right.
"Say you're in a [chemical] plant and there's a snake on the floor. What are you going to do? Call a consultant? Get a meeting together to talk about which color is the snake? Employees should do one thing: walk over there and you step on the friggin� snake." - Jean-Pierre Garnier, CEO of Glaxosmithkline, June 2006

Sponsored Links