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Before you post a questions I recommend that you download the pdf document about the subject you want to ask a question about and read it carefully.
If you don't want to return to this webpage to often I recommend that you subscribe to the feed. More information about RSS and subscriptions is found here.
Looking forward to help you.
posted by Anders Nielsen at
1:59 AM
4 Comments:
what would be the ionic strenth of say 100mM Glucose? where there is no charge?
For any standard calculations glucose is not considered charged - and should not contribute to the overall ionic strength of the solution.
How do I attack this problem? I want to compare the effect of adding 1mmol of HCL to 100 ml of 0.2M acetate buffer at two different starting pH's. (pKa of acetate buffer =4.7
Initial pH = 4.7
Initial pH = 5.7
Thank you
Hi Debra,
I will make a Q&A section a.s.a.p. and answer your question thoroughly with calculations and everything.
However:
1) set up a charge balance with Na+, Ac-, H+ and a Cl- and adjust your Cl- so that the charge balance is zero.
2) Change your Cl- with the equivalent of the HCl you add!
3) adjust H+ so that your new charge balance is zero.
Since this is difficult I'll give you the short answer here. The buffer solution a pH=4.7 changes the most in pH as at pH=4.7 you are closer to the equivalence point of the buffer.
At pH 4.7 adding the HCl will change the pH notably to 4.61. At pH 5.7 you will hardly see any change at all.
But get back to pHscale.net because soon a thorough explanation is given
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