Predict the stronger acid in each pair: (a) HCl or HF; (b) H3 PO4 or H3 AsO4 j(𝐜) HBrO3 or HBrO2

step 1 Chapter 16, probably 88 from chemistry, the central science. Today we're going to be predicting

Predict the stronger acid in each pair: (a) HCl or HF; (b)...

Predict the stronger acid in each pair: (a) HCl or HF; (b) $\mathrm{H}_{3} \mathrm{PO}_{4}$ or $\mathrm{H}_{3} \mathrm{AsO}_{4 j}(\mathbf{c}) \mathrm{HBrO}_{3}$ or $\mathrm{HBrO}_{2} ;(\mathbf{d}) \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}$ or $\mathrm{HC}_{2} \mathrm{O}_{4}^{-} ;$ (e) benzoic acid $\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)$ or phenol $\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\right).$

Key Concepts

Oxoacid Structure and Acidity

Oxoacids contain hydrogen, oxygen, and another element (the central atom) and their acid strength depends on the electronegativity of the central atom and the number of oxygen atoms bonded to it. More electronegative central atoms and a greater number of oxygen atoms generally increase the acid’s strength by stabilizing the conjugate base through electron withdrawal.

Periodic Trends in Acidity

Periodic trends, such as variations in electronegativity and atomic size, play a significant role in acid strength. For instance, acids containing heavier halogens generally form weaker bonds with hydrogen, facilitating easier proton release. This understanding helps predict trends in acidity across different elements.

Resonance Stabilization

Resonance stabilization involves the delocalization of electrons over several atoms or bonds, distributing the negative charge more evenly in the conjugate base. This delocalization reduces the energy of the conjugate base, thereby enhancing the acid's strength by making deprotonation more favorable.

Acid Strength

Acid strength refers to the tendency of an acid to donate its proton (H?) in solution. This concept is quantitatively described by the acid dissociation constant (Ka); a larger Ka indicates a stronger acid. Understanding acid strength is essential in comparing different acids in various chemical contexts.

Conjugate Base Stability

The stability of the conjugate base formed after an acid donates a proton is a key determinant of acid strength. A more stable conjugate base, often achieved through factors such as delocalization of the negative charge or inductive effects, enhances the acid’s ability to release its proton, making the acid stronger.

Transcript

00:01 Chapter 16, probably 88 from chemistry, the central science.

00:05 Today we're going to be predicting which acid in the group is the strongest acid.

00:10 So what we're first going to be looking at is the different acids and then how they differ and then being able to use different trends from the period table to help be able to answer our questions.

00:24 So the first one we have is hcl and hf and hcl and hf.

00:31 Hf are both part of the halogen group.

00:35 And so the thing that we're going to be using here to help determine which one is the stronger acid is highly dependent on the atomic radius of our fluorine and our chlorine.

00:49 And whenever you look at our trend, we have an atomic radius trend that goes to the left and down.

00:56 And so fluorine is at the top and then cl is right underneath it.

01:00 And so since we know that, then we know that chlorine has a larger atomic radius.

01:12 And so therefore, whenever you have to bond to the hydrogen also has a larger bond distance.

01:25 And so therefore, it is easier for the hydrogen and the chlorine to break than it is in the hydrogen fluorine.

01:31 So our answer for a is going to be h .cl is the strongest acid.

01:38 So in b, we have h3p -o -4 and h -3 -a -s -o -4.

01:51 And to help determine which one of these acids is the strongest acid, we need to look at a couple of things.

01:59 One is to look at the oxidation, what's going on, but they have the same things.

02:10 The next thing is to look at the electro -negativity of the central component of your compound...

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