Does water/ or solid have concentration?

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SUMMARY

The discussion centers on the concept of concentration in relation to water and solids in chemical solutions. Participants clarify that the concentration of pure solids and solvents, such as water, is often considered constant and is thus omitted from equilibrium expressions like Kw = Kc[H2O] = [H][OH]. This simplification is based on the understanding that the concentration of these components does not significantly change during reactions, allowing for a more straightforward calculation of equilibrium constants.

PREREQUISITES
  • Understanding of chemical equilibrium concepts
  • Familiarity with equilibrium constants (Kc and Kw)
  • Basic knowledge of concentration and molarity
  • Awareness of the role of solvents in chemical reactions
NEXT STEPS
  • Research the derivation of equilibrium constants in chemical reactions
  • Study the implications of omitting solids and solvents in equilibrium calculations
  • Learn about the behavior of water as a solvent in various chemical reactions
  • Explore advanced topics in chemical thermodynamics
USEFUL FOR

Chemistry students, educators, and professionals interested in chemical equilibrium and reaction dynamics will benefit from this discussion.

mcato_O
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does water/ or solid have concentration?

does water/ or solid have concentration?
Why do we just ignore the concentration of solid or solution solvent and replace it as one M? I always thought the reason is because the concentration of solid or water solvent does not change much so in practice we just move it to the Kc side” such as Kw = Kc[H2O]=[H][OH]? Now I am not so sure
 
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