Hbr or hi which is stronger acid

We seek only the relative acidity of the hydrohalides, not the absolute value. Continued below. At this juncture we have a fluorine and iodine atom in the gas phase. Could someone please explain this to me. That means that stronger acids will release more hydrogens than weaker acids, and HI will release more hydrogens than fluorine because fluorine is smaller and its hold on the electrons in hydrogen is tighter because of its small size.

HF is a weak acid because it does not disassociate as easily in water the H-F bond is harder to break. As you go down the halogens, the atom sizes become bigger and the bond between the element and H become weaker. These are more likely to disassociate in water. An oxoacid sometimes called an oxyacid is an acid that contains oxygen. To be more specific, an oxoacid is an acid that:. Sulphuric acid : Drops of the concentrated oxoacid sulfuric acid sulphuric acid rapidly dehydrate a piece of cotton towel.

These acids can be arranged in order of their pK a values and, by extension, their relative strengths:. Recall that smaller values of pKa correspond to greater acid strength. Therefore, HOCl is the strongest acid and HOI is weakest, and acid strength decreases as the central halogen descends on the periodic table.

Because Cl is the most electronegative, it draws the bulk of the electrons in the HOCl molecule toward itself; because H and Cl are on opposite ends of the molecule, Cl pulls at the electrons in the H-O bond, thereby weakening it. Consider the family of chlorooxoacids, which are arranged below in order of pK a values:. The strongest acid is perchloric acid on the left, and the weakest is hypochlorous acid on the far right.

Notice that the only difference between these acids is the number of oxygens bonded to chlorine. As the number of oxygens increases, so does the acid strength; again, this has to do with electronegativity.

Carboxylic acids are an important subclass of organic oxoacids, characterized by the presence of at least one carboxyl group. Carboxylic acids are the most common type of organic acid. Acids with two or more carboxyl groups are called dicarboxylic, tricarboxylic, etc.

The simplest dicarboxylic example is oxalic acid COOH 2 , which is just two connected carboxyls. Mellitic acid is an example of a hexacarboxylic acid. Other important natural examples include citric acid in lemons and tartaric acid in tamarinds.