**MODIFIED**

To write the Henderson-Hasselbalch equation for Tris Buffer.

And my answer:

Tris·HCl + H2O ↔ Tris·Cl + + H3O+

**My question is**Did I get that right? But somehow I am wondering if it is supposed to be TrisClˉ for the conjugate base instead.

Secondly,

Is there any molecular formula for Tris·HCl & Tris·Cl?

I have searched on Wikipedia and it is actually C4H11NO3 for Tris. So is it actually

C4H11NO3HCl for Tris·HCl and

C4H11NO3Cl for Tris·Cl?

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As for the second question.

Find the total concentration of a buffer of 100mL with the ionic strength of 0.05M.

I have actually worked this out using the formula n = cV

∴ c = n/V

c = 0.05M/0.1L

= 0.5mol

Did I get the right formula? I am quite confused with the whole molarity thing and am trying to fix up the pieces of the different formulas that I can actually use.

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Thanks for your help :]

Hey guys

Would appreciate if anybody could help me with the following:

- Chemical equation for Tris Buffer (Tris HCl/Tris Base)?
- What is the final conc of the buffer (Tris HCl/Tris Base pKa 8.1, Buffer of ionic strength 0.05M, pH 8.5)

Thanks in advance!