If p Kb for fluoride ion at 25^∘ C is 10.3, the ionization constant of hydrofluoric acid in wate

step 1 Hello everyone so in this question P KB value of P KB value of of fluoride ion is 10 .3 okay we

If p Kb for fluoride ion at 25^∘ C is 10.3, the ionization...

If $\mathrm{p} K_{\mathrm{b}}$ for fluoride ion at $25^{\circ} \mathrm{C}$ is $10.3$, the ionization constant of hydrofluoric acid in water at this temperature is $(\log 2=0.3)$
(a) $2 \times 10^{-4}$
(b) $2 \times 10^{-3}$
(c) $2 \times 10^{-5}$
(d) $5 \times 10^{-11}$

Key Concepts

Relationship between Ka and Kb

For conjugate acid-base pairs, the product of the acid dissociation constant (Ka) and the base dissociation constant (Kb) equals the ionization constant of water (Kw). This relationship, expressed as Ka × Kb = Kw, enables the calculation of one constant if the other is known, linking the behavior of acids and their conjugate bases.

Ionization Constants (Ka and Kb)

Ionization constants, Ka for acids and Kb for bases, quantify the degree to which an acid or base dissociates in water. These constants allow chemists to evaluate the strength of acids and bases, predict the direction of equilibrium, and calculate pH values in various chemical environments.

Water Ionization Constant (Kw)

The water ionization constant (Kw) reflects the extent of water's self-ionization into hydrogen ions (H?) and hydroxide ions (OH?). It is a pivotal constant in aqueous chemistry that serves as a reference point for calculating the dissociation constants of acids and bases and understanding pH regulation in water.

Acid-Base Equilibrium

Acid-base equilibrium describes the dynamic balance in aqueous solutions where acids donate protons (H?) and bases accept them. It forms the foundation for understanding how substances ionize and establish equilibrium in solution, and it is quantified using equilibrium constants such as Ka and Kb.

Conjugate Acid-Base Pairs

Conjugate acid-base pairs are formed when an acid donates a proton to become its conjugate base, or when a base accepts a proton to become its conjugate acid. This concept underscores the inverse relationship between the strengths of acids and bases, as a strong acid has a weak conjugate base and vice versa.

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