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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Sheryl Mackie on March 14, 2006, 08:07:09 PM

Title: Buffer pH
Post by: Sheryl Mackie on March 14, 2006, 08:07:09 PM

An initial buffer solution has a pH of 9.25 and .200M NH4Cl and .200M NH3. What is the pH after adding .0050 mol NaOH?

I think charts have to be made.

Thank you,

Sheryl

Title: Re:Buffer pH
Post by: Mitch on March 14, 2006, 08:30:42 PM

http://www.chembuddy.com/?left=pH-calculation&right=pH-buffers-henderson-hasselbalch (http://www.chembuddy.com/?left=pH-calculation&right=pH-buffers-henderson-hasselbalch)

Title: Re:Buffer pH
Post by: Borek on March 16, 2006, 03:57:51 AM

Quote from: Sheryl M. on March 14, 2006, 08:07:09 PM

An initial buffer solution has a pH of 9.25 and .200M NH4Cl and .200M NH3. What is the pH after adding .0050 mol NaOH?

Assume NaOH reacted stoichiometrically with NH₄⁺, the use Henderson-Hasselbalch equation using link Mitch posted ;)