Use the following acid ionization constants to identify the correct decreasing order of base strengths for the conjugate bases. $\mathrm { HF } \quad K _ { \mathrm { a } } = 7.2 \times 10 ^ { - 4 }$
$\mathrm { HNO } _ { 2 } \quad K _ { \mathrm { a } } = 4.5 \times 10 ^ { - 4 }$
$\mathrm { HCN } \quad K _ { \mathrm { a } } = 6.2 \times 10 ^ { - 10 }$

Question

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The strength of a conjugate base is inversely related to the strength of its acid. The weaker the acid, the stronger its conjugate base. HCN has the smallest $ K_a $, making CN^- the strongest base, followed by HNO₂ and HF.

Use the Following Acid Ionization Constants to Identify the Correct HFKa=7.2×10−4\mathrm { HF } \quad K _ { \mathrm { a } } = 7.2 \times 10 ^ { - 4 }HFKa​=7.2×10−4

Use the Following Acid Ionization Constants to Identify the Correct $\mathrm { HF } \quad K _ { \mathrm { a } } = 7.2 \times 10 ^ { - 4 }$