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Basic concepts in Acids and Bases:

 

Arrhenius concept

The concept is based on the presence of  and   ions in the aqueous solution of the given substance. It states that an acid gives  ions in its aqueous solution whereas a base gives ions in its aqueous solution.  

 

Bronsted-Lowery concept

This concept is based on the capacity of a substance to  give or accept the  ions. It is not based on the presence of aqueous solution. 

 

Conjugate acid-base

 A Bronsted acid can give  ion and results in the formation of a conjugate base of it whereas a Bronsted base can accept  ion and results in the formation of conjugate acid of it.  

 

Lewis acid-base concept

The Lewis acid - base concept was based on the transfer of electrons during the chemical reactions. A substance is said to be Lewis acid if the substance can accept the electrons whereas a substance is known as Lewis base if it can donate its lone pairs of electrons or extra electrons. 

 

Acid and base dissociation constant 

The dissociation of weak acids shows equilibrium and can be represented with the help of dissociation constant. 

 

 

 

pH of solution

The concentration of in a solution can be expressed with the help of pH value which ranges from 0 to 14. The pH value 0 to 7 stands for acidic whereas the pH value 7-14 stands for basic solution. The pH value 7 stands for neutral solution. The mathematical expression for pH is: 

 

 

 

Buffer solutions

Buffer solutions are the solutions which show resistance in change in pH value even after addition of a little amount of acid or base to the solution.   

 

Hasselbach-Henderson equation

The equation is used to calculate the pH and pKa value of buffer solution. The mathematical expression of equation can be written as:

 

 

 

 

Sample Acid and Base Problems: 

 

Question 1: Calculate the pH value of 0.025 M solution of HCl. 

Solution:

 

Answer: pH = 1.6 

 

Question 2:  Which combination can act as a buffer solution? 

Strong acid + Strong base
Weak acid + Weak base 
Weak acid + Salt of weak acid with strong base 
Strong acid + Salt of weak acid with strong base 

Solution: A mixture of weak acid with salt of that acid with strong base acts as a buffer solution. 
 

Answer: c) 
 

Question 3: Identify the Lewis base in the given substances.

Ammonia 
Hydrogen chloride 
Ammonium chloride 
Ethanol 
 
Solution: A Lewis base is the substance that can give its extra pair of electrons or lone pair of electrons. In the given substances, ammonia must be Lewis base as N contains one lone pair of electrons. 

Answer: a) 

 

 

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FAQs

 

 

What is an acid and what is a base? 

 

An acid can be defined as the substance that can give H⁺ ions in their aqueous solution whereas a base the substance can give OH⁻ ions in their aqueous solution. 

 

What is the difference between an acid and a base?

 

                 Acid                               Base
It can give  H⁺ ions. It can give OH⁻ ions.
It has a sour taste.  It has a bitter taste. 
Example: Citric acid  Example: Sodium hydroxide 

 

 

What are 5 examples of bases?

 

  • Sodium hydroxide 
  • Potassium hydroxide 
  • Calcium hydroxide 
  • Magnesium hydroxide 
  • Baking soda 

 

What are 3 types of acids?

 

  • Tartaric acid 
  • Sulfuric acid 
  • Nitric acid

 

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