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### When to use the Henderson-Hasselbalch Equation

Posted: **Sun Dec 06, 2015 10:41 am**

by **004624886**

Can I use the Henderson-Hasselbalch equation when I have a weak acid that is being titrated by a strong base, but not all the way to the stoichiometric point? I guess my real question would be, is the HH equation valid when the volume (and thus molarity) of a system is changing (if I were to calculate the molarities of the weak acid and its conjugate base after the addition of the titrant), or does it only apply to systems with unchanging volume where the added strong base is a salt dissolved in the solution?

### Re: When to use the Henderson-Hasselbalch Equation

Posted: **Sun Dec 06, 2015 11:02 am**

by **Chem_Mod**

Yes, you can use it in this situation. Be careful when determining your concentrations of the conjugate acid/base pair.

### Re: When to use the Henderson-Hasselbalch Equation

Posted: **Fri Dec 02, 2016 8:37 pm**

by **Martha Xuncax 3G**

So we will have the option of using the Henderson-Hasselbalch equation or the ice box on the final?

### Re: When to use the Henderson-Hasselbalch Equation

Posted: **Sun Jun 03, 2018 11:44 pm**

by **juliaschreib1A**

This equation is used for estimating the pH of a buffer solution.

### Re: When to use the Henderson-Hasselbalch Equation

Posted: **Sun Jun 03, 2018 11:46 pm**

by **Mariah Guerrero 1J**

Will we have to know this equation for the final? We haven't learned about it in lecture yet, right?