Why is hocl more acidic than hobr

It makes sense when we think about it. In these terms, chlorine is more Electra negative than bro me. So chlorine is gonna better stabilize the contra get base here than bro Mean will um, And so Ah, a s'more stable, stronger, confident base equals a stronger acid. Um And so that explains why H o. L is a stronger asked than h o b r. We're comparing at acids of the type hz, where the acidity is gonna increase along a row and down a column vs, um, these H o halogen acids, where we need to take the stability of the contra, get bases into account and therefore the electro negativity of each halogen.

Uh and so that's the answer to chapter to problem number Although the addition of one equivalent of HX … Which is the stronger acid of each of the following pairs of acids? Explain … Sulfuric acid is a weaker acid than hydrochloric acid.

Yet hydrogen chloride… Explain the following statement. View Full Video Already have an account? Ian K. Problem 19 Medium Difficulty Explain the apparent paradox. Answer If the conjugate base is stable then the corresponding acid would be stronger. View Answer. Topics Liquids. Organic Chemistry Chapter 2 Acids and Bases. Discussion You must be signed in to discuss. Top Chemistry Educators Theodore D. Carleton College. Lizabeth T. Allea C. University of Maryland - University College.

Jacquelin H. Brown University. Chemistry Bootcamp Lectures Liquids - Intro A liquid is a nearly incom…. Recommended Videos Problem Video Transcript This is the answer to chapter to problem number 19 from the Smith Organic Chemistry textbook. Numerade Educator. Liquids - Intro A liquid is a nearly incompressible fluid that conforms to the shape of its …. Although the addition of one equivalent of HX …. Explain …. The same reasoning applies for both HBr and HI. These acids are even stronger than HCl because the Br — and I — ions are even larger.

As such, the H-Br and H-I bonds are even weaker, and these compounds also readily dissociate in solution. Binary acids are one of two classes of acids, the second being oxoacids or oxyacids , which consist of hydrogen, oxygen, and a third element, which is often a non-metal. 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. Salts and esters of carboxylic acids are called carboxylates. When a carboxyl group is deprotonated, its conjugate base, a carboxylate anion, forms.

Carboxylate ions are resonance stabilized, and this increased stability makes carboxylic acids more acidic than alcohols. Carboxylic acids can be seen as reduced or alkylated forms of the Lewis acid carbon dioxide; under some circumstances they can be decarboxylated to yield carbon dioxide.