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Ionic Equilibrium (11th) formulas

Master Ionic Equilibrium (11th) through 22 JEE Advanced-level formulas, systematically structured with every variable spelled out. Revise concept-wise, identify the areas where you need improvement, and focus your preparation with greater precision.

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Ionic Equilibrium (11th), every formula

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Ionic product of water
$K_{w} = [H^{+}] [O H^{-}] = 1 0^{- 14} (2 5^{\circ} C)$
Q1MCQKw
The ionic product of water at $25^{\circ}$C is:
- A
  $10^{-14}$
- B
  $10^{-7}$
- C
  $10^{14}$
- D
  $1$
pH
$pH = - lo g [H^{+}]$
pOH
$pOH = - lo g [O H^{-}]$
pH + pOH
$pH + pOH = 14$
Acid dissociation constant
$K_{a} = \frac{[ H ^{+} ] [ A ^{-} ]}{[ H A ]}$
Q1MCQKa
The acid dissociation constant is:
- A
  $\dfrac{[H^{+}][A^{-}]}{[HA]}$
- B
  $\dfrac{[HA]}{[H^{+}][A^{-}]}$
- C
  $[H^{+}][A^{-}]$
- D
  $\dfrac{[H^{+}]}{[HA]}$
Base dissociation constant
$K_{b} = \frac{[ B H ^{+} ] [ O H ^{-} ]}{[ B ]}$
Q1MCQKb
The base dissociation constant is:
- A
  $\dfrac{[BH^{+}][OH^{-}]}{[B]}$
- B
  $\dfrac{[B]}{[BH^{+}][OH^{-}]}$
- C
  $[BH^{+}][OH^{-}]$
- D
  $\dfrac{[OH^{-}]}{[B]}$
Ka × Kb
$K_{a} \times K_{b} = K_{w}$
Q1MCQKa × Kb
For a conjugate acid–base pair, $K_a\times K_b$ equals:
- A
  $K_w$
- B
  $1$
- C
  $K_a$
- D
  $K_w^{2}$
Ostwald's dilution law
$K_{a} = \frac{α ^{2} C}{1 - α} \approx α^{2} C$
Q1MCQOstwald
Ostwald's dilution law for a weak acid is:
- A
  $K_a\approx\alpha^{2}C$
- B
  $K_a=\alpha C$
- C
  $K_a=\dfrac{\alpha}{C}$
- D
  $K_a=\alpha^{2}$
Degree of dissociation
$α = \frac{K _{a}}{C}$
Q1MCQDegree of dissociation
The degree of dissociation of a weak acid is:
- A
  $\sqrt{\dfrac{K_a}{C}}$
- B
  $\dfrac{K_a}{C}$
- C
  $K_a C$
- D
  $\sqrt{K_a C}$
[H⁺] of a weak acid
$[H^{+}] = K_{a} C$
Q1MCQ[H⁺] weak acid
The $[H^{+}]$ of a weak acid of concentration $C$ is:
- A
  $\sqrt{K_a C}$
- B
  $K_a C$
- C
  $\dfrac{K_a}{C}$
- D
  $K_a$
pKa
$p K_{a} = - lo g K_{a}$
Henderson equation (acid buffer)
$pH = p K_{a} + lo g \frac{[ salt ]}{[ acid ]}$
Q1MCQHenderson (acid)
The Henderson equation for an acidic buffer is:
- A
  $\text{pH}=\text{p}K_a+\log\dfrac{[\text{salt}]}{[\text{acid}]}$
- B
  $\text{pH}=\text{p}K_a-\log\dfrac{[\text{salt}]}{[\text{acid}]}$
- C
  $\text{pH}=\text{p}K_a$
- D
  $\text{pH}=\log[\text{salt}]$
Henderson (base buffer)
$pOH = p K_{b} + lo g \frac{[ salt ]}{[ base ]}$
Q1MCQHenderson (base)
The Henderson equation for a basic buffer gives:
- A
  $\text{pOH}=\text{p}K_b+\log\dfrac{[\text{salt}]}{[\text{base}]}$
- B
  $\text{pH}=\text{p}K_b$
- C
  $\text{pOH}=\text{p}K_a$
- D
  $\text{pOH}=\log[\text{base}]$
Solubility product
$K_{s p} = [A^{+}]^{x} [B^{-}]^{y}$
Q1MCQKsp
The solubility product of $A_xB_y$ is:
- A
  $[A^{+}]^{x}[B^{-}]^{y}$
- B
  $[A^{+}][B^{-}]$
- C
  $[A^{+}]^{y}[B^{-}]^{x}$
- D
  $[A^{+}]+[B^{-}]$
Ksp of a salt AB
$K_{s p} = S^{2}$
S = molar solubility
Q1MCQKsp of AB
For a salt AB of solubility $S$, $K_{sp}$ is:
- A
  $S^{2}$
- B
  $S$
- C
  $4S^{3}$
- D
  $2S$
Ksp of AB₂
$K_{s p} = 4 S^{3}$
Q1MCQKsp of AB₂
For a salt $AB_2$ of solubility $S$, $K_{sp}$ is:
- A
  $4S^{3}$
- B
  $S^{3}$
- C
  $S^{2}$
- D
  $2S^{2}$
Common-ion effect
$added common ion suppresses dissociation/solubility$
Q1MCQCommon-ion effect
Adding a common ion to a weak electrolyte:
- A
  suppresses its dissociation
- B
  increases dissociation
- C
  has no effect
- D
  changes $K_a$
Hydrolysis (salt of weak acid)
$pH = 7 + \frac{1}{2} (p K_{a} + lo g C)$
Q1MCQSalt hydrolysis
The pH of a salt of a weak acid and strong base is:
- A
  $>7$ (basic)
- B
  $<7$ (acidic)
- C
  $=7$
- D
  $0$
Degree of hydrolysis
$h = \frac{K _{w}}{K _{a} C}$
Q1MCQDegree of hydrolysis
The degree of hydrolysis of a salt of a weak acid is:
- A
  $\sqrt{\dfrac{K_w}{K_a C}}$
- B
  $\sqrt{\dfrac{K_a}{C}}$
- C
  $\dfrac{K_w}{K_a}$
- D
  $K_a C$
Buffer at half-neutralization
$pH = p K_{a}$
Q1MCQHalf-neutralization
At half-neutralization of a weak acid, the pH equals:
- A
  $\text{p}K_a$
- B
  $7$
- C
  $14$
- D
  $0$
Neutral solution
$[H^{+}] = [O H^{-}] = 1 0^{- 7} M$
Precipitation condition
$ionic product > K_{s p} \Rightarrow precipitation$
Q1MCQPrecipitation
A precipitate forms when the ionic product is:
- A
  greater than $K_{sp}$
- B
  less than $K_{sp}$
- C
  equal to $K_{sp}$
- D
  zero

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Ionic Equilibrium (11th) formulas

Ionic Equilibrium (11th), every formula

Ionic product of water

pH

pOH

pH + pOH

Acid dissociation constant

Base dissociation constant

Ka × Kb

Ostwald's dilution law

Degree of dissociation

[H⁺] of a weak acid

pKa

Henderson equation (acid buffer)

Henderson (base buffer)

Solubility product

Ksp of a salt AB

Ksp of AB₂

Common-ion effect

Hydrolysis (salt of weak acid)

Degree of hydrolysis

Buffer at half-neutralization

Neutral solution

Precipitation condition

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