Equilibrium - Notes, Topics, Formula, Books, FAQs

A state in which the rates of the forward and reverse reactions are equal and the concentrations of the reactants and products remain constant. Equilibrium is a dynamic process – the conversions of reactants to products and products to reactants are still going on, although there is no net change in the number of reactant and product molecules. Equilibrium is of two type chemical equilibrium and ionic equilibrium.

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This Story also Contains

1. Important Topics Of Chemical Equilibrium
2. Applications of Equilibrium Constant:
3. Factors affecting chemical equilibrium:
4. Ionic Equilibrium in Solution
5. Important Topics Of Ionic Equilibrium
6. Overview Of Ionic Equilibrium
7. Ionization of Acids and Bases
8. Ionic Product of Water
9. The pH Scale
10. The relation between Ka and Kb
11. Buffer Solutions
12. How to prepare for Equilibrium?

Important Topics Of Chemical Equilibrium

Law Of Mass Action:

It states that “the rate at which a substance reacts is directly proportional to its activity and the rate at which substances react together is directly proportional to the product of their activity each raised to a power which is equal to the corresponding stoichiometric number is called Law Of Mass Action

Equilibrium Constant:

Equilibrium Constant is the ratio of the rate of forward and backward reaction at a particular temperature or it is the ratio of active masses of the reactants to that of active masses of products at a particular temperature raised to their stoichiometric coefficients.

Relation Between Kp And Kc:

The relationship between the concentrations or partial pressures of reactants and products in a chemical reaction at equilibrium is called Relation Between Kp And Kc.

Degree Of Dissociation:

Degree Of Dissociation is the extent to which any reactant gets dissociated. Due to dissociation, the total number of moles at equilibrium can be determined. Knowing the number of moles at equilibrium, the observed molar mass can be calculated.

Le Chatelier's Principles On Equilibrium:

It is defined as the ratio of the concentration of products to the concentration of the reacting species raised to their stoichiometric coefficient at any point of time other than the equilibrium stage is called Le Chatelier's Principles On Equilibrium.

Overview Of Chemical Equilibrium

Take a reaction as follows:

Equilibrium Constant is given by the following equation:

Chemical equilibrium occurs when both the reactions(forward and backward) are occurring at equal rates.

The chemical equilibrium and its laws have various real-life applications as mentioned below:

• Hemoglobin and oxygen exist in equilibrium in the blood by the reaction:
  Hb(aq) + 4O2 Hb(O2)4(aq).
  As a result, a person tends to feel light-headed at higher altitudes.
  
  

• Nitrogen and other gases are dissolved in our blood, now if the diver comes up too fast from the deep ocean, suddenly there is an equilibrium shift takes place thus develops nitrogen bubbles in the blood which causes severe pain and death.
  
  

EQUILIBRIUM IN PHYSICAL PROCESS

Some of the phase processes of equilibrium are as follows:

• Solid-liquid equilibrium:
  For example, ice and water are at equilibrium at only one temperature is called a normal melting point.

• Liquid-gas equilibrium:
  For example, rate of evaporation = rate of condensation
  H₂O(l) ? H₂O(vap)

• Solid-gas equilibrium:
  This process is also called sublimation
  e.g. sublimation of camphor

Solid-liquid equilibrium:
Law of mass action: The equilibrium concentrations of reactants and products may vary, but the value K_c remains constant.

Characteristics of K_c

1. The reaction equilibrium can be obtained from both directions.

2. K_c is a function of temperature.

3. K_c is independent of the initial concentration of reactants and products.

4. If the K_c value is

• << 1, the equilibrium lies to the right and the reaction mixture contains mostly products.

• 0.10<Kc<10, the mixture contains a proportionate amount of reactants and products.

• >> 1, the equilibrium lies to the left and the reaction mixture contains mostly reactants.

Homogeneous Equilibria
When all the reactants and the products in the equilibrium are in the same phase, then this equilibrium is known as homogeneous equilibrium. For example:

In this reaction, all these reactants are in the gaseous phase, thus it is a homogeneous equilibrium

Heterogeneous Equilibria
When the reactants are in different phases, then this system of equilibrium is known as the heterogeneous equilibrium. For example,

In this reaction, all these reagents are in different phases, thus it is a heterogeneous equilibrium.

Applications of Equilibrium Constant:

• Predicts the extent of reaction, which gives the degree of the disappearance of reactants.
• Predicts the direction of the reaction.
• Calculating the equilibrium constant, which gives the relative amount of reactants and products.

Reaction Quotient (Q):
The reaction value obtained when we substitute reactant and product concentrations into the equilibrium expression.

1. If Q>K the reaction shifts towards the reactants side.

2. If Q<K the reaction shifts towards the products side.

3. If Q+K no shift occurs (equilibrium achieved).

Factors affecting chemical equilibrium:

• Lechatlier ’s Principle: It states that changes in temperature, pressure, volume or concentration of a system will result in predictable and opposing changes in the system in order to achieve a new equilibrium state. It can be used to select the optimum conditions to form a substance.
• Changes in temperature:
  Endothermic(H>0): R+ Heat Products.
  Exothermic(h<0): R Products+ Heat
• Effect of catalyst:
  The Catalyst increases the rate of reaction for both forward and reverse reactions. The catalyst does not affect the equilibrium concentration of both reactants and products. So the value K_c doesn’t change.

Ionic Equilibrium in Solution

Ionic equilibrium is the study of equilibrium between the ions. All those substances that are converted into ions in solution are classified into categories i.e. strong electrolytes and weak electrolytes. Strong electrolytes are those that are completely dissociated into ions and conduct greater electricity, while weak electrolytes are those that are partially ionized in solutions and conduct smaller electricity. Acids, bases, and salts are either weak electrolytes or strong electrolytes. In the case of weak electrolytes, the equilibrium is established between the ions and non-ionized molecules.

Important Topics Of Ionic Equilibrium

Bronsted Lowry And Lewis Acid-base Theory:

According to Bronsted Lowry And Lewis Acid-base Theory, an acid is a substance that can donate a proton and a base is a substance that can accept a proton

Ionization Of Acids And Bases:

The process by which a neutral molecule breaks down into charged ions when exposed to a solution is known as compound ionization. When an acid dissociates into an aqueous medium to produce the hydrogen ion H⁺ and bases are the hydroxide compounds that give OH− ions on dissociation in water called Ionization Of Acids And Bases

Ka And Kb Relationship:

Ka and Kb are equilibrium constants that indicate the relative amounts of products and reactants at equilibrium.

Buffer Solution

A solution whose pH does not change very much when H⁺(H₃O⁺) or OH^- are added to it is referred to as a Buffer Solution.

Common Ion Effect:

The Common Ion Effect is defined as the phenomenon where the solubility of an ionic compound decreases in a solution that already contains one of the ions present in the compound.

PH Of Acids And Bases:

A solution having a PH between 0 to 7 is called an acid and a solution whose PH ranges in between 7 and above up to 14 is called a base and the pH in between 0 to 14 is called Ph Of Acids And Bases.

Solubility And Solubility Product:

The maximum amount of a particular solute in grams, which can dissolve in 100 grams of solvent at a given temperature is called Solubility And Solubility Product is the product of the molar concentrations of ions of an electrolyte in a saturated solution at a particular temperature.

Salt Hydrolysis:

When a salt is added to water ions of the salt interact with water to cause acidity or basicity in an aqueous solution. This ionic interaction is called Salt Hydrolysis.

Overview Of Ionic Equilibrium

Ionization of Acids and Bases

As already mentioned, some acids and bases are strong in nature and some are weak in nature. When a strong acid dissociates in the aqueous medium then it forms its conjugate base, these conjugate bases are always weak in nature. Similarly, with strong bases, their conjugate acids in solutions are always weak. For weak acids and bases, their conjugates bases and acids, respectively are always strong in nature.

The acid-base dissociation equilibrium of an acid HA is given as below:

an acid-base conjugate acid conjugate base

Ionic Product of Water

In pure water, one water molecule donates a proton and acts as an acid and another water molecule accepts a proton and acts as a base. The equilibrium reaction goes as follows:

The dissociation constant for this equilibrium reaction is given as follows:

can be eliminated since it is liquid, thus the ionic product of water or K_w is given as:

After calculations, the value of K_w is equal to = 1 x 10^-14M²

Thus any aqueous solution is acidic, basic, or neutral is determined by the conditions below:

• For acidic:
• For neutral:
• For basic:

The pH Scale

The hydronium ion concentration of any solution is expressed in a logarithmic scale, then it is known as pH scale. Thus, the pH of any solution is defined as the negative logarithm value of hydrogen ion concentration. Mathematically, it can be expressed as follows:

Now as we know, the pure water has hydrogen ion concentration = 10^-7, therefore, pH of water = 7
Thus we can conclude as follows:

• Acidic solution has pH < 7
• Basic solution has pH > 7
• Neutral solution has pH = 7

From the above calculations, it has been found that:

The relation between K_a and K_b

K_a and K_b are the strengths of acidic and basic solutions respectively. Now, for every net reaction, the equilibrium constant is equal to the product of the added reactions.
Thus, K_a x K_b = K_w
Therefore, pK_a + pK_b = pK_w = 14

Buffer Solutions

These are the solutions that resist the change in pH if the solution is diluted or some small amounts of alkali or acid are added. For example, a mixture of acetic acid and sodium acetate is a buffer solution with pH equal to 4.75.

How to prepare for Equilibrium?

• This chapter is a part of Physical chemistry. This chapter is one of the most important chapters of the complete chemistry syllabus. Its concepts, laws, numerals and graphs all are important both for the basic foundation of chemistry and for scoring good marks in the examination.

• Before reading this chapter, first, you must have a basic knowledge of the mole concept.

• In this chapter, all the equations and formulae are very simple and easy to remember.

• Rest this chapter is very simple, just be regular and be consistent in your numerical practice.

Prescribed Books for Equilibrium

First, you must finish the class XI NCERT book and solve each and every example and unsolved question given in it. Then for advanced level preparation like JEE and NEET, you must follow R.C. Mukherjee and O.P. Tandon. You must definitely solve the previous year's papers. Meanwhile, in the preparation, you must continuously write the mock tests for the depth of knowledge. Our platform will help you with a variety of questions for deeper knowledge with the help of videos, articles, and mock tests.

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