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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