Introduction To Aromatic Carboxylic Acid

Introduction:

Aromatic Carboxylic acid (COOH): Any of a class of organic compounds in which a carbon (C) atom is bonded or attached to an oxygen (O) atom by a hydroxyl group (-oh) and to a double bond by a sigma bond. A fourth bond links the carbon atom to a(H) hydrogen atom or to some anthor combining group. The (COOH) carboxyl group is so-named because of the (C=O) carbonyl group and (OH) hydroxyl group. Acidity is The main chemical characteristic of the carboxylic acids. They are generally have higher acidicty than other organic compounds containing (_OH) hydroxyl groups but are generally weaker than the familiar mineral acids (e.g. hydrochloric acid, HCl, etc.). Carboxylic acids occur mainly in nature. Fatty acids are components

In h2o, a hydrogen ion is shifted from the carboxyl group to a h20 molecule. example, with the ethanoic acid, and ethanoate formed together with , H3O+ (hydronium ion) .

These are therefore weak acids.

The pH of carboxylic acid solutions:

The pH mainly depends on both the concentration of the acid and how easily it loses hydrogen ions from the carboxyl group .

Ethanoic acid is typical of the acids where the carboxyl group is attached to a alkyl group. Typical lab solutions have pH's with a range from 2 - 3 , depending on the concentrations.

Methanoic acid is rather stronger than the other acids, and solutions have pH's of the range of( 0.5 pH )units less than ethanoic acid of the same concentration.

Benzoic

Acidic character surrounded by benzoic acids, which have different electron releasing group .

Factors that affect’s Acidity

-Bronsted acids are proton donors.

-Lewis acids are electron pair acceptors. Converse: proton acceptor =Bronsted base, Lewis base = electron pair donor.

1. A conjugate base is what you obtain when you remove a proton from a compound. For instance, HO (-) is the conjugate base of water. O (2- ) is the conjugate base of HO (-).on the other hand , conjugate acids are what you obtain when you add a proton to a compound. The conjugate acid of water is hydronium ion .

2. Quick quiz: is( pH 1) acidic or basic? The PKa is equal to pH in that low denote strong acids. This is why pKa is based on the equilibrium.

3. Finally , anything which stabilizes the conjugate base will change the acidity.

Here are some factors :

Factor #1 – Charge.

Removal of a proton, decreases the charge on an atom or molecule by one unit.

This isbecause of the easy to do when an atom bears a charge of +1 firstly, and becomes progressively more difficult as the overall charge becomes (-). The acidity trends reflect