Chemistry
I'm not getting the right answers for the pH, [H2A], and [HA^-] in part a (0.135 M solution for H2A) For H2A, I did 3.9E-2=x^2/(.135-x) Using the quadratic formula: x^2+.039x-.005265=0 x=.06725 [H^+]=[HA^-]=.06725 M pH=-log(.06725)=1.17 Finding [H2A]=.135 M-.06725 M=.06775...
Chemistry
Given a diprotic acid, H2A, with two ionization constants of Ka1=3.9E-2 and Ka2=5.9E-8. Calculate the pH and molar concentration of each protonated form for a 0.135 M solution of: (a) H2A (b) NaHA (c) Na2A
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