Ionic Equilibrium Class 11: Acid-Base Theories

What is the formula to calculate pH from pOH?

Which components are essential for a solution to act as a buffer?

What does buffer capacity refer to?

How can pH be calculated for a buffer solution using the Henderson-Hasselbalch equation?

What is the optimal pH range for a buffer to effectively resist pH changes?

Which statement accurately describes the Arrhenius Theory of acids and bases?

What is the relationship between solubility and the solubility product constant (Ksp)?

Which best describes the Common Ion Effect?

What is pH defined as?

How do you calculate the solubility of a salt from its Ksp value?

Which of the following correctly defines a weak acid in relation to pH calculations?

What distinguishes the Brønsted-Lowry theory from the Arrhenius theory?

Which statement is true regarding the Lewis Theory of acids and bases?

Calculating pH from pOH

pH + pOH = 14

Buffer Components

A weak acid and its conjugate base
Or a weak base and its conjugate acid

Buffer Capacity

The amount of acid or base a buffer can neutralize before a significant change in pH occurs

Henderson-Hasselbalch Equation

pH = pKa + log([A-]/[HA])
Where:
- pKa: The negative logarithm of the acid dissociation constant (Ka)
- [A-]: The concentration of the conjugate base
- [HA]: The concentration of the weak acid

Optimal Buffer pH Range

A buffer works best within ± 1 pH unit of its pKa

Arrhenius Theory of Acids and Bases

Acids produce hydrogen ions (H+) in water, and bases produce hydroxide ions (OH-) in water

Solubility & Ksp Relationship

Ksp is the product of the ion concentrations at equilibrium in a saturated solution
A higher Ksp value indicates greater solubility

Common Ion Effect

The solubility of a sparingly soluble salt decreases when a soluble compound containing a common ion is added to the solution

pH Definition

pH is the negative logarithm of the hydrogen ion concentration ([H+]) in a solution

Calculating Salt Solubility from Ksp

Use the equilibrium constant expression for the dissolution of the salt and solve for the solubility of the salt

Weak Acid Definition

A weak acid ionizes only partially in solution, resulting in a pH higher than that of a strong acid at the same concentration

Brønsted-Lowry vs. Arrhenius Theory

Brønsted-Lowry theory defines acids as proton donors (H+) and bases as proton acceptors, whereas Arrhenius theory focuses on the production of H+ or OH- in aqueous solutions

Lewis Theory of Acids and Bases

Lewis acids accept electron pairs, and Lewis bases donate electron pairs. This definition encompasses both proton-based interactions and electron-pair sharing interactions.

This quiz explores the foundational concepts of ionic equilibrium and various acid-base theories as part of the Class 11 chemistry curriculum. It covers the Arrhenius, Brønsted-Lowry, and Lewis theories, along with the solubility product and its significance. Test your understanding of these critical chemical principles.