The increasing order of basic strength of Cl, CO3^2, CH3 COO, OH, F is (1) Cl<F<CH3 COO<CO3^2<OH

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The increasing order of basic strength of Cl, CO3^2, CH3...

The increasing order of basic strength of $\mathrm{Cl}, \mathrm{CO}_{3}^{2}$, $\mathrm{CH}_{3} \mathrm{COO}, \mathrm{OH}, \mathrm{F}$ is (1) $\mathrm{Cl}<\mathrm{F}<\mathrm{CH}_{3} \mathrm{COO}<\mathrm{CO}_{3}^{2}<\mathrm{OH}$ (2) $\mathrm{Cl}^{-}<\mathrm{F}^{-}<\mathrm{CO}_{3}^{2-}<\mathrm{CH}_{3} \mathrm{COO}^{-}<\mathrm{OH}^{-}$ (3) $\mathrm{CHI}_{3} \mathrm{COO}<\mathrm{Cl}<\mathrm{F}<\mathrm{CO}_{3}^{2}<\mathrm{OH}$ (4) $\mathrm{F}<\mathrm{CO}_{3}^{2}<\mathrm{Cl}<\mathrm{CII}_{3} \mathrm{COO}<\mathrm{OII}$

The increasing order of basic strength of $\mathrm{Cl}, \mathrm{CO}_{3}^{2}$, $\mathrm{CH}_{3} \mathrm{COO}, \mathrm{OH}, \mathrm{F}$ is
(1) $\mathrm{Cl}<\mathrm{F}<\mathrm{CH}_{3} \mathrm{COO}<\mathrm{CO}_{3}^{2}<\mathrm{OH}$
(2) $\mathrm{Cl}^{-}<\mathrm{F}^{-}<\mathrm{CO}_{3}^{2-}<\mathrm{CH}_{3} \mathrm{COO}^{-}<\mathrm{OH}^{-}$
(3) $\mathrm{CHI}_{3} \mathrm{COO}<\mathrm{Cl}<\mathrm{F}<\mathrm{CO}_{3}^{2}<\mathrm{OH}$
(4) $\mathrm{F}<\mathrm{CO}_{3}^{2}<\mathrm{Cl}<\mathrm{CII}_{3} \mathrm{COO}<\mathrm{OII}$

Key Concepts

Periodic Trends in Halide Ions

Halide ions exhibit trends in basicity that are influenced by their electronegativity and size. Generally, as one moves from chloride to fluoride in solution, subtle differences in solvation and electronegativity can affect their behavior as bases. Understanding these trends helps in comparing the intrinsic basic strengths of halide ions in various chemical environments.

Conjugate Acid–Base Relationship

This concept means that the strength of a base is directly related to the acidity of its conjugate acid. A weak conjugate acid (one with a high pKa) gives rise to a strong base, while a strong acid (with a low pKa) forms a very weak base. Therefore, comparing the pKa values of the conjugate acids allows chemists to predict the relative basicity of their corresponding bases.

pKa and Base Strength

The pKa value of a conjugate acid is a quantitative measure of its acidity. A high pKa indicates a weak acid, which corresponds to a stronger conjugate base. By evaluating the pKa values of the acids corresponding to various anions, one can order the bases from weakest to strongest based on the increasing basic strength reflected by their conjugate acid’s pKa.

Resonance Stabilization and Basicity

Resonance stabilization can significantly affect basicity. When an anion is stabilized by resonance, its negative charge is delocalized over multiple atoms, making it less reactive toward protonation. Therefore, anions with resonance stabilization tend to be weaker bases compared to those without such stabilization, as the delocalized charge diminishes the species’ tendency to attract a proton.

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