Why Is the pH of Hydroxylamine Less Than 7?

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SUMMARY

The pH of hydroxylamine is calculated to be 6.04, despite it being a base, due to its equilibrium constant (Kb) of 1.10 x 10^-8. The discussion highlights the importance of using the correct Henderson-Hasselbalch equation, particularly in buffer regions, to avoid erroneous results. For initial pH calculations, it is recommended to utilize the equilibrium constant equation instead of the Henderson-Hasselbalch equation.

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What is the pH of hydroxylamine? From my calculations, it is 6.04. But it is a base. So why is it less than 7?! For calculations I just used the Henderson-Hasselbalch equation. The Kb is 1.10*10^-8, and when 0 ml of titrant has been added, the pH would be 6.04.
 
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MaddenDude said:
What is the pH of hydroxylamine?
That will depend on the concentration.

From my calculations, it is 6.04.
How? Care to post your "calculations" here?
 
You've got to use the right henderson-hasselbach equation (in buffer regions), for instance, if you were to use the Kb in the acid h-h equation, you would get erroneous results.

In addition, you don't want to use the h-h equation for the initial pH, simply work with the equilibrium constant equation.
 

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