Understanding Acid Solutions: How to Reach 10^-14

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SUMMARY

The discussion centers on the equilibrium constant of water autodissociation, specifically the value of 10^-14 at 25°C. This constant represents the product of the concentrations of hydrogen ions (H+) and hydroxide ions (OH-) in pure water. In an acidic solution, the concentration of H+ ions is increased, which inversely suppresses the concentration of OH- ions, maintaining the equilibrium constant at 10^-14. This relationship is fundamental to understanding acid-base chemistry.

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  • Basic understanding of acid-base chemistry
  • Familiarity with chemical equilibrium concepts
  • Knowledge of ion concentration calculations
  • Understanding of water autodissociation
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Chemistry students, educators, and professionals interested in acid-base reactions and the properties of aqueous solutions.

PainterGuy
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hello everyone,

i read it somewhere:--

In such a solution at 25C, the product of concentration of H+ ions with the concentration of OH- ions must be 10^-14. In an acid solution, by forcing a high concentration of H+ ions, you necessarily suppress the concentration of OH- ions.

what is this saying? how do one get 10^-14?

i am grateful for any help you can give me. many thanks.

cheers
 
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painterguy said:
what is this saying? how do one get 10^-14?

10-14 is a value of an equilibrium constant of the water autodissociation:

H2O <-> H+ + OH-

and its value is determined experimentally.

See also water ion product.
 

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