chemistry

glycine and lysine, have the following values of the relevant acid dissociation constants (pKa)
glycine, pKa=2.35
lysine,pKa=10.79

For an aqueous solution of glycine alone, calculate the value of pH at which the ratio of the concentration of neutral glycine zwitterions to the concentration of protonated cation is 102.

asked by Will
  1. This tutorial may help.
    http://www.chem.uiuc.edu/CLCtutorials/104/AminoAcidTitrations/SeeIt.html
    I would use the Henderson-Hasselbalch equation and substitute into the log term either 1/100 or 100/1 depending upon which way you want to write it.

    posted by DrBob222
  2. Here is the titration curve for glycine.
    https://www.google.com/search?q=titration+amino+acids&client=firefox-a&hs=ha9&rls=org.mozilla:en-US:official&channel=sb&tbm=isch&tbo=u&source=univ&sa=X&ei=jjr9U9jcKdH9yQTljIH4Dw&ved=0CCYQsAQ&biw=1024&bih=609#facrc=_&imgdii=_&imgrc=HsTtE2YEggYW1M%253A%3BEMsM7v-IV9G1fM%3Bhttp%253A%252F%252Fwww.chem.fsu.edu%252Fchemlab%252Fbch4053l%252Fcharacter%252Ftitration%252Findex_clip_image006.jpg%3Bhttp%253A%252F%252Fwww.chem.fsu.edu%252Fchemlab%252Fbch4053l%252Fcharacter%252Ftitration%252F%3B369%3B275

    posted by DrBob222
  3. thank you I'm looking into this albeit totally lost atm

    posted by Will
  4. 9.78+log10(1/102)
    =7.77

    sounds good?

    posted by Will
  5. Nevermind, I did it, I should be paying you for all this help ;)

    I had to take other pk

    2.35+log10(102)
    =4.35

    posted by Will

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