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Weak Acid and Base Equilibria

AP Chemistry· difficulty 4/5

For NH4+_4^+ (conjugate acid of NH3_3), Ka=5.6×10−10K_a = 5.6\times10^{-10}. What is KbK_b for NH3_3?

  • A

    1.8×10−51.8\times10^{-5} (Kw/KaK_w/K_a)

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  • B

    1.0×10−141.0\times10^{-14}

  • C

    5.6×10−45.6\times10^{-4}

  • D

    5.6×10−105.6\times10^{-10}

Explanation

Conjugate pair: Ka⋅Kb=Kw=10−14K_a \cdot K_b = K_w = 10^{-14}. Kb=10−14/(5.6×10−10)=1.8×10−5K_b = 10^{-14}/(5.6\times10^{-10}) = 1.8\times10^{-5}.

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