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Weak Acid and Base Equilibria

AP Chemistry· difficulty 4/5

For H3_3PO4_4, Ka1=7.5×10−3K_{a1} = 7.5\times10^{-3}, Ka2=6.2×10−8K_{a2} = 6.2\times10^{-8}, Ka3=4.8×10−13K_{a3} = 4.8\times10^{-13}. The pH of 0.10 M H3_3PO4_4 is dominated by which dissociation?

  • A

    Ka3K_{a3} (smallest)

  • B

    Ka2K_{a2}

  • C

    Sum of all three

  • D

    Ka1K_{a1} (much larger than the others)

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Explanation

Successive dissociations get weaker (negative ion holds the next H+^+ tighter). Ka1K_{a1} dominates pH; subsequent contribute negligibly.

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