What is the chemical definition of a base?
A molecule that accepts H+ ions.
There are about 5 definitions. The three most popular ones in use today (tomorrow may be a different story) are
1. The Arrhenius theory-- A base is a substance that produces hydroxide ions when placed in water solution.
2. The Bronsted-Lowry theory-- A base is a substance that accepts protons.
3. The Lewis theory-- A base is a substance that donates electrons.
Not many use the Arrhenius theory today--it's a shame too for it is so simple. Th Bronsted-Lowry theory is used widely in freshman an analytical chemistry; the Lewis theory is used widely in organic chemistry.
The chemical definition of a base refers to a substance that can accept protons (H+) or donate pairs of electrons during a chemical reaction. Bases are substances that, when dissolved in water, increase the concentration of hydroxide ions (OH-) in the solution.
One way to determine the chemical definition of a base is by looking at its behavior in water. Bases typically have a bitter taste, feel slippery to touch, and can conduct electricity when dissolved in water. Another way to identify a base is by using pH indicators, which change color when the pH of a solution becomes more basic.
Moreover, the Arrhenius theory defines a base as a substance that dissociates in water to produce hydroxide ions (OH-). For example, when sodium hydroxide (NaOH) dissolves in water, it dissociates into sodium ions (Na+) and hydroxide ions (OH-). The hydroxide ions are responsible for the basicity of the solution.
In summary, the chemical definition of a base is a substance that accepts protons or donates pairs of electrons during a chemical reaction, resulting in an increase in the concentration of hydroxide ions (OH-) in a solution.