Solutions: Equilibrium of Salts in Solution

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The discussion focuses on the equilibria involving sulfur species in solution, particularly how the initial concentration of sulfur affects the equilibrium concentrations of various species. It emphasizes that while the initial concentration of sulfur may be the same across different compounds (like SO2, Na2SO3, or NaHSO3), the total amounts of hydrogen and oxygen will differ based on the specific species added, impacting the overall equilibrium. The conversation also highlights the importance of charge and mass balance equations, noting that the presence of counter ions like Na+ must be considered in charge balance calculations. Additionally, the participants discuss the implications of assuming water's concentration as constant versus variable, and how this affects the modeling of equilibria in dilute versus non-dilute solutions. Ultimately, the discussion underscores the complexity of chemical equilibria and the need for careful consideration of all variables involved.
  • #31
Come on, try to work out something yourself!
Big-Daddy said:
What do you mean? Can you just write the one equation?

The problem with Na+ conservation is that Na+ is also contributed to by another salt.

Of course, but ##c_0(NaHSO3)## is known as it is completely dissolved, at least, that's what you were assuming.
 
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  • #32
I'm sorry, I've tried and I don't know the answer.
 
  • #33
Set up the conservation equation for Na and use it to eliminate c0(Na2SO3)=n0(Na2SO3)/V, where n0(Na2SO3) is the total amount of dissolved Na2SO3) (i.e. c0(Na2SO3) is an additional variable in your system).
 
  • #34
Ok, what if I then added K2SO3 up to saturation? Is it

Mass Balance for S: (1/2) * [K+] + (1/2) * ([Na+] - c0[NaHSO3]) + c0[NaHSO3] = [SO2] + [HSO3-] + [SO32-]
 

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