Isohydric solutions are the solutions having the same...

Isohydric solutions are the solutions having the same concentration of hydronium ion. If $0.2 \mathrm{M}-$ HA solution is isohydric with $4 \times 10^{-4} \mathrm{M}-\mathrm{HCl}$ solution, then $K_{\mathrm{b}}$ of $\mathrm{A}^{-}$ is (a) $8 \times 10^{-7}$ (b) $1.25 \times 10^{-8}$ (c) $1.25 \times 10^{-6}$ (d) $8 \times 10^{7}$

Isohydric solutions are the solutions having the same concentration of hydronium ion. If $0.2 \mathrm{M}-$ HA solution is isohydric with $4 \times 10^{-4} \mathrm{M}-\mathrm{HCl}$ solution, then $K_{\mathrm{b}}$ of $\mathrm{A}^{-}$ is
(a) $8 \times 10^{-7}$
(b) $1.25 \times 10^{-8}$
(c) $1.25 \times 10^{-6}$
(d) $8 \times 10^{7}$

Key Concepts

Relationship Between K? and K_b

For a conjugate acid-base pair, the acid and base dissociation constants are interrelated by the ion product of water (K_w), expressed as K? × K_b = K_w. This relationship allows one to determine the base strength (K_b) from the known acid strength (K?) when the ionization of water is taken into account.

Conjugate Base and Base Dissociation Constant (K_b)

The conjugate base (A?) of a weak acid reacts with water to form the acid (HA) and hydroxide ions (OH?). The base dissociation constant (K_b) measures the strength of this reaction. It is a fundamental concept for understanding the basicity of the conjugate base in solution.

Isohydric Solutions

Isohydric solutions are those that have the same concentration of hydronium ions (H?O?) regardless of the nature of the acid present. This concept is useful for comparing properties of weak and strong acids when they produce the same acidic environment.

Acid Equilibrium

Acid equilibrium refers to the reversible dissociation process of an acid (HA) in water where it partially ionizes to form hydronium ions and its conjugate base (A?). Understanding this equilibrium helps in determining the acid’s strength via its dissociation constant.

Acid Dissociation Constant (K?)

The acid dissociation constant, K?, quantifies the extent of ionization of an acid in solution, defined by the ratio [H?][A?] to [HA]. It is a critical concept for assessing the relative strength of weak acids and predicting the concentration of ions in solution.

Transcript

Please give Ace some feedback