Acid and base definition

In this article we are going to focus on the basics of acid and bases. So one of the frist thing that you need to be able to do is you need to be able to identify an acid and base. If you are given the chemical form of it. 

Acids typically have a hydrogen in front of them. So HCl that's hydrochloric acid HF Hydrofluoric acid as you see. There is a hydrogen infront of. It or acidic HC2H3OH those are acids.

Bases typically have a hydroxide ion like KOH, NaOH, those are bases. If you see a hydrogen next to a metal like sodium hydride. Then it is a base not an acid but if the hydrogen is attached to  a non metal technically acid. Acid so whenever hydrogen has a positive charge. It is an acid  but it hydrogen has a like a negative charge then it's a base. Acids tend to be positively charged. Bases are usually negatively charged.

Arrhenius Or lrenaeus definition of acids


Acids are basically there's substances that release H+ ions into the solution.
Hydrogen ions are equivalent to hydronium in water. This really does not exist by itself in water in fact. It is actually bonded to water and so it exists as H3O + . A base releases hydroxide ions in syst solution while acids release H+ions into solution. So keep that in mind know you also need the Bronsted - Lowry definition of acids.

Bronsted - Lowry definition of acids 

Acids are proton donors bases are proton acceptors. So let's say if we put hydrochloric acid in water what's going to happen .HCl is the Bronsted lowry acid. H2O is the lowry base. The acid is a proton donor. So HCl is going to lose the hydrogen and turn in to chloride the base is a proton acceptor. Water is going to accept the H+ ion and it's going to convert it into the hydronium ion is called the conjugate acid because we added a hydrogen to water to make it and this is the conjugate base because we took away a hydrogen to make it the conjugate base and the base turns in to the conjugate acids in the course of acid and base reaction. Let's look at another example Ammonia when it reacts with water it produces NH4 and OH-.
NH3 + H2O -----------> NH4 +      +    OH-

This example identify the acid base.

The conjugate base so notice that NH3. It gained the hydrogen turning into NH4 So therefore is the proton acceptor which means NH3 is the base. In this example water lost the hydrogen so water was the proton donor. It gave away hydrogen which makes it . The acid now the base is always going to turn into the conjugate acid because we should the hydrogen to it. So NH4+ is the conjugate acid which means hydroxide has to be the conjugate base because water lost the hydrogen to make it. Now let's say it you are given water and you want to write the conjugate acid of water and the same time the conjugate base what is the conjugate acid of water.