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To write the Henderson-Hasselbalch equation for Tris Buffer.
And my answer:
Tris·HCl + H2O ↔ Tris·Cl + + H3O+
My question isDid 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!