Equilibrium-Ionic NEET Mindmaps PDF and Formulas

Equilibrium-Ionic NEET Mindmap Concepts

Concept

Explanation from Mindmap

Electrolyte

Substances that allow an electric current to flow when they are dissolved in water. Strong electrolytes break up completely into ions. Weak electrolytes only break up partly into ions.

Ionic Equilibrium

A balance that is reached in a weak electrolyte solution. This balance is between the part of the substance that has not broken up (unionised) and the part that has broken up into ions (ionised).

Acid-Base Concepts

Arrhenius Concept: An acid is a substance that produces Hydrogen ions in water. A base is a substance that produces Hydroxide ions in water. Bronsted-Lowry Concept: An acid is a proton donor. A base is a proton acceptor. Conjugate pairs are formed when an acid gives a proton to a base. 

🔹 Formula: Acid strength is often measured by $K_a$ = (H⁺ × conjugate base) ÷ unionised acid. Base strength by $K_b$ = (OH⁻ × conjugate acid) ÷ unionised base.

Value of Ionic Product

This value shows the combined amount of Hydrogen ions and Hydroxide ions in water. It is a constant value for pure water at a fixed temperature. At 25 degrees Celsius, this value is $1.0 × 10^{-14}$. 

🔹 Formula: $K_w$ = [H⁺] × [OH⁻].

pH Scale

The pH scale is a way to measure how acidic or basic a solution is. A neutral solution, like pure water, has a pH of 7. Solutions with a pH value less than 7 are acidic. Solutions with a pH value greater than 7 are basic. 🔹 Formula: pH = −log[H⁺]. pOH = −log[OH⁻]. Also, pH + pOH = 14 (at 25°C).

Hydrolysis of Salts

This is a chemical reaction where a salt reacts with water. The result of this reaction can be an acidic, basic, or neutral solution. For example, a salt made from a strong acid and a strong base will form a neutral solution when it reacts with water. 

🔹 Formula (simple words): For hydrolysis constant $K_h$ = $K_w / (K_a$ or $K_b)$ depending on type of salt.

Solubility Product

This concept is used to find the maximum amount of an ion that can dissolve in a saturated solution. It helps in calculating the equilibrium concentration, which is important for understanding how a sparingly soluble salt dissolves.

 🔹 Formula : $K_{sp}$ = multiply concentrations of all ions in saturated solution. Example: For AgCl → [Ag⁺] × [Cl⁻].

Acid Strength

Measures how easily an acid can give away its proton (Hydrogen ion). Strong acids break up completely in water. The stronger an acid is, the weaker its conjugate base will be.

Common Ion Effect

A process where the breaking up of a weak electrolyte is reduced or suppressed by adding another substance that shares a common ion with it. For example, adding sodium acetate (a salt) to acetic acid (a weak acid) reduces the breakup of the acetic acid.

Equilibrium-Ionic NEET Mindmap Formulas

Topic

Formula

Ionic Product of Water ($K_w$)

[H⁺] × [OH⁻] = $1 × 10^{-14}$ (at 25°C).

pH Formula

pH = −log[H⁺].

pOH Formula

pOH = −log[OH⁻].

pH and pOH Relation

pH + pOH = 14 (at 25°C).

Degree of Dissociation (α)

α = (moles ionized ÷ total moles).

Acid Dissociation Constant ($K_a$)

$K_a$ = ([H⁺] × [Conjugate base]) ÷ [Unionized acid].

Base Dissociation Constant ($K_b$)

$K_b$ = ([OH⁻] × [Conjugate acid]) ÷ [Unionized base].

Strength Relation

Higher $K_a$ → Stronger Acid. Higher $K_b$ → Stronger Base.

Solubility Product ($K_{sp}$)

Multiply concentrations of all ions in saturated solution.

Buffer Equation (Henderson–Hasselbalch)

pH = pKa + log (salt ÷ acid).