A base is defined in chemistry as a substance that reacts with acids to form a salt and releases hydroxide ions in an aqueous solution. Furthermore, the base accepts protons or donates electrons.
Table of Contents
Important Characteristics of Bases
- Bases can be used to neutralize acids. A harmless water molecule is formed when a base, usually OH–, accepts a proton from an acid. It is known as neutralization.
- A base causes litmus paper to turn blue. It turns the methyl orange indicator yellow and the phenolphthalein indicator pink. In the presence of a base, bromothymol blue remains blue.
- The pH of basic solutions is greater than 7.
- Basis reacts violently with acids and organic matter, resulting in chemical burns.
- The ions dissociated from an aqueous base solution or molten bases solution conduct electricity.
- Lime is a base that is used by farmers to help neutralize acidic soil.
- Rubbing baking soda solution, a base, on the sting of an ant can help relieve the pain because it neutralizes the formic acid in the sting.
| Common Strong bases | Formula |
| Sodium hydroxide | NaOH |
| Calcium hydroxide | Ca(OH)2 |
| Potassium hydroxide | KOH |
| Barium hydroxide | Ba(OH)2 |
Types of Base
- Strong Base: Strong bases are those that completely dissociate their ions into water or any other compound capable of removing a proton from any weak acid. KOH and NaOH are two examples.
- Weak Base: Weak bases are substances that do not completely dissociate their ions into the water.
- Super Base: These bases are formed by alkali metals and their conjugate acid and are superior to strong bases.
- Neutral Base: Neutral bases are substances that form a bond with neutral acid.
Frequently Asked Questions
1. What are the different definitions of acids and base?
Acids and bases are classified into three types.
The Arrhenius definition is the most straightforward, stating that acids are compounds that increase proton concentration in solution, whereas bases are compounds that increase hydroxide concentration in solution. Hydrogen is always present in Arrhenius acids, and hydroxide groups are always present in Arrhenius bases.
Proton donation is central to Brnsted-Lowry definitions. Bronsted-Lowry acids are compounds that donate protons, whereas Brnsted-Lowry bases accept protons.
The donation or acceptance of an electron pair is referred to as Lewis acids and bases. Lewis bases give up an electron pair, while Lewis acids accept one.
2. What is the definition of the base in terms of Ph?
In chemistry, a base has a pH (on the pH scale) of 8-14. It is a substance capable of accepting protons. An alkali is a base that dissolves in water.
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