Give Arrhenius and Bronsted definition of acid and

The Arrhenius and Bronsted-Lowry definitions are two commonly used definitions to describe acids and bases.
According to the Arrhenius definition:
$Anacidisasubstancethatproduceshydrogenions(H^{+})inaqueoussolution.$
$Abaseisasubstancethatproduceshydroxideions(O{H}^{-})inaqueoussolution.$
In the Arrhenius definition, the focus is on the ions produced in solution. Acids release hydrogen ions (H+) and bases release hydroxide ions (OH-) when dissolved in water.
On the other hand, the Bronsted-Lowry definition provides a broader understanding of acids and bases:
$Anacidisasubstancethatdonatesaproton(H^{+}).$
$Abaseisasubstancethatacceptsaproton(H^{+}).$
In the Bronsted-Lowry definition, the focus is on the transfer of protons (H+ ions). Acids are proton donors, and bases are proton acceptors.
The Bronsted-Lowry definition is considered more useful in describing acid-base properties for several reasons:
1. It is more inclusive: The Bronsted-Lowry definition encompasses a broader range of substances that can exhibit acid-base behavior. It is not limited to aqueous solutions like the Arrhenius definition, as it can be applied to reactions in non-aqueous solvents or even gas-phase reactions.
2. It allows for amphoteric substances: According to the Bronsted-Lowry definition, substances can act as both acids and bases. This concept of amphoteric behavior is crucial in understanding the behavior of substances like water, which can donate a proton as an acid (H2O → H+ + OH-) and accept a proton as a base (H2O + H+ → H3O+).
3. It emphasizes the role of proton transfer: The Bronsted-Lowry definition focuses on the transfer of protons, which is a fundamental concept in acid-base chemistry. It provides a more comprehensive understanding of acid-base reactions and allows for the analysis of acid-base equilibria and reaction mechanisms.
Overall, the Bronsted-Lowry definition is more versatile and applicable in a wide range of contexts, making it more useful in describing acid-base properties than the Arrhenius definition.