Homework Statement
If the Tris buffer was exactly pH=9.0, calculate expected pH value after addition of 1 ml of 0.05 HCl.
Buffer: 4 ml of 0.01M Tris, pH 9.0
HCl: 1 ml of 0.05M HCl
Homework Equations
H-H: pH=pKa+log[A-]/[HA]
The Attempt at a Solution
9.0=8.21+log[A-]/[HA]...
I would need .005 mols, (0.1M Tris)x(0.05L)=.005. But then how do I go back to ml from here? And where does the 1.0M Tris base come in, since that is the solution I am diluting to get the 0.1M solution?
EDIT: I think I figured it out. Would it be (1.0M Tris)(X L)=(0.1M Tris)(.05L), so I would...
Homework Statement
Calculate the theoretical volumes of 1.0 M Tris base, 1.0 N HCL or 0.2 NaOH, and water needed to prepare 50 ml of a 0.1 M Tris buffer pH 9.0. pKa of Tris: 8.21 Homework Equations
Henderson-Hasselbalch: pH=pKa + log[A-]/[HA]The Attempt at a Solution
Honestly, I don't even know...