How to calculate pH of two weak acids

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SUMMARY

This discussion focuses on calculating the pH of a mixed solution containing 0.200M of two weak acids, HA and HB, with dissociation constants (Ka) of 1.0 x 10^-5 and 1.0 x 10^-6, respectively. The total concentration of the acids in the solution is 0.4M, and it is crucial to recognize that the acids have different Ka values, which affects the pH calculation. The correct approach involves using the individual dissociation constants to determine the contribution of each acid to the overall pH.

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  • Understanding of weak acid dissociation and equilibrium
  • Knowledge of the Henderson-Hasselbalch equation
  • Familiarity with pH calculation methods
  • Basic algebra for solving equilibrium expressions
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how to calculate the pH of a mixed solution containg 0.200M HA and 0.2 HB
ka of HA =1.0^10-5
KA OF HB = 1.0^-6
 
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Not only you have ignored template and not showed any effort, you also listed both acids as if their Ka were identical and equal 1.

So - you may safely assume you have 0.4M solution of acid with Ka=1.
 

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