Strength of Acid
Acids are defined as substances with a pH less than 7.0. As the amount of H+ ions in the solution increases, the value decreases. Strong acids are compounds that rapidly release H+ ions or are completely ionizable in solution. As a result, strong acids have a lower pH value, close to 0 to 1. The higher the concentration of H+ ions in the solution, and hence the stronger the acid, the lower the pH value.
For example, Hydrochloric acid, Sulfuric acid, Nitric acid, Perchloric acid, Chloric acid, etc.
Strength of Weak Acid
A weak acid is one that does not entirely ionize in solution. In low quantities, it releases the H+ ion, resulting in a pH range of 5 to 7. Formic acid (HCOOH), acetic acid (CH3COOH), and many more acids are examples.
Acids and Bases
An acid is a substance that is capable of donating a proton (hydrogen ion) to another substance. A base is a molecule able to donate OH- ion/strong>. Acidic substances are usually identified by their sour taste.
Acids have a sour taste and are corrosive i.e. exposure to acid on human skin can cause blisters. Some examples of acids are HCl, H2SO4, and others.
Let’s learn more about acids and bases, their properties, theories, and others in this article.
Table of Content
- What are Acids?
- What are Bases?
- Acid Bases Titration
- pH of Acid and Base
- Difference between Acids and Bases
- Acid-Base Reaction
- Acid-Base Indicator Definition