The dissociation constants of formic and acetic acids are 1.77 ×10^-4 and 1.75 ×10^-5, respectiv

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The dissociation constants of formic and acetic acids are...

The dissociation constants of formic and acetic acids are $1.77 \times 10^{-4}$ and $1.75 \times 10^{-5}$, respectively (a) Formic acid is $3.18$ times stronger than acetic acid, at equal concentration. (b) Acetic acid is $3.18$ times stronger than formic acid, at equal concentrations. $\begin{array}{lllll}\text { (c) Formic acid is } 10.11 & \text { times }\end{array}$ stronger than acetic acid, at equal concentrations. (d) Formic acid is $10.11$ times stronger than acetic acid, at different concentrations

The dissociation constants of formic and acetic acids are $1.77 \times 10^{-4}$ and $1.75 \times 10^{-5}$, respectively
(a) Formic acid is $3.18$ times stronger than acetic acid, at equal concentration.
(b) Acetic acid is $3.18$ times stronger than formic acid, at equal concentrations.
$\begin{array}{lllll}\text { (c) Formic acid is } 10.11 & \text { times }\end{array}$ stronger than acetic acid, at equal concentrations.
(d) Formic acid is $10.11$ times stronger than acetic acid, at different concentrations

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Key Concepts

Acid Dissociation Constant (Ka)

The acid dissociation constant, Ka, is a quantitative measure of an acid's strength in solution. It represents the equilibrium constant for the dissociation of an acid into its conjugate base and a proton, indicating the extent to which the acid ionizes. A larger Ka value signifies a greater degree of ionization and, consequently, a stronger acid.

Relationship Between Ka and Acid Strength

The strength of an acid is directly tied to its dissociation constant; acids with higher Ka values dissociate more completely in solution, releasing more protons. This fundamental relationship enables the comparison of acid strengths by examining their respective Ka values.

Comparative Analysis of Acid Strength

Comparing the acid strengths involves evaluating the ratio of their dissociation constants. By analyzing these ratios, one can determine which acid is stronger under the same conditions, as a higher Ka value implies a stronger acid even if the concentrations are identical.

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