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11 Nov 2019
H3PO4 has three acidic protons with the following Ka values: Ka1 = 7.1 x 10-3 Ka2 = 6.3 x 10-8 = 4.5 x 10-13 If you have this acid in a solution with a pH-5 what is the predominate form of the compound in solution? 3- PO4 H2PO4 2- No. Compare the pKa values of each acidic proton dissociation with the pH in the problem. pKa1 -log(Ka1) 2.15 and pKa2log(Ka2) = 7.20 and pKa3 =-log(Kag) = 12.35. H3PO4
H3PO4 has three acidic protons with the following Ka values: Ka1 = 7.1 x 10-3 Ka2 = 6.3 x 10-8 = 4.5 x 10-13 If you have this acid in a solution with a pH-5 what is the predominate form of the compound in solution? 3- PO4 H2PO4 2- No. Compare the pKa values of each acidic proton dissociation with the pH in the problem. pKa1 -log(Ka1) 2.15 and pKa2log(Ka2) = 7.20 and pKa3 =-log(Kag) = 12.35. H3PO4
Reid WolffLv2
30 May 2019