The Naked Scientists

The Naked Scientists Forum

Author Topic: precipitates and salts  (Read 2337 times)

Offline matt1234

  • First timers
  • *
  • Posts: 1
    • View Profile
precipitates and salts
« on: 19/05/2006 01:20:01 »
how do i know if a precipitate will form from a mixture.
for example will a precipitate form from this hypothetical mixture,
Na2X (2.5x10^-5M) and MCl (1.4x10^-5M) (Ksp of M2X = 5.6x10^-14)
i just dont get it. thanks if anyone can help.
matt:)


 

Offline DrDick

  • Sr. Member
  • ****
  • Posts: 162
    • View Profile
Re: precipitates and salts
« Reply #1 on: 25/05/2006 20:18:21 »
Ksp (given) for M2X = [M+]^2[X-] (at equilibrium)
also
Qsp = [M+]^2[X-] (at given conditions)

If Q = K, then you are at equilibrium, and have a saturated solution - nothing should happen.
If Q < K, then no equilibrium will take place.  Concentration is less than the saturation limit.
If Q > K, then solution has too many dissolved ions, and they will precipitate.

DrDick
 

The Naked Scientists Forum

Re: precipitates and salts
« Reply #1 on: 25/05/2006 20:18:21 »

 

SMF 2.0.10 | SMF © 2015, Simple Machines
SMFAds for Free Forums