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Chapter 16: Problem 60

How does the strength of an oxoacid depend on the electronegativity and oxidation number of the central atom?

Short Answer

Expert verified
The strength of an oxoacid depends on the electronegativity and oxidation number of the central atom. As the electronegativity and oxidation number increase, the strength of the oxoacid also increases. This is due to an increase in the ability of the central atom to attract bonding pair of electrons (electronegativity) and the ability of the central atom to stabilize the resulting conjugate base after the acid donates an H+ ion (oxidation number).

Step by step solution

01

Understand the Basics of Oxoacids

Oxoacids are acids that contain hydrogen, oxygen, and another element. When considering the acid strength, the higher the electronegativity of the central atom, the stronger the acid. This is because electronegativity is a measure of the ability of an atom to attract a bonding pair of electrons.
02

Understand the Impact of Electronegativity on Acid Strength

When the central atom is highly electronegative, it draws electron density away from the Oxygen-Hydrogen bond (O-H bond). This makes the O-H bond weaker and easier to break, hence making the oxoacid stronger.
03

Understand the Effect of Oxidation Number on Acid Strength

A higher oxidation number of the central atom means more oxygen atoms can be bonded. With these extra oxygen atoms, they can aid in further withdrawing the electron density from the O-H bond, making the O-H bond easier to break. This results in the oxoacid being stronger. So, the oxidation number not only affects the number of oxygen atoms that can be attached but also the strength of the acid.
04

Summary

So in summary, both an increase in electronegativity and oxidation number of the central atom in an oxoacid will boost its acidic strength.

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Most popular questions from this chapter

Prediet the \(\mathrm{pH}(>7,<7,\) or \(\approx 7)\) of the aqueous solutions containing the following salts: (a) \(\mathrm{KBr}\) (b) \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) (c) \(\mathrm{BaCl}_{2}\) (d) \(\mathrm{Bi}\left(\mathrm{NO}_{3}\right)_{3}\).

Hydrocyanic acid (HCN) is a weak acid and a deadly poisonous compound that, in the gaseous form (hydrogen cyanide), is used in gas chambers. Why is it dangerous to treat sodium cyanide with acids (such as HCl) without proper ventilation?

To which of the following would the addition of an equal volume of \(0.60 \mathrm{M} \mathrm{NaOH}\) lead to a solution having a lower \(\mathrm{pH} ?\) (a) water, (b) \(0.30 \mathrm{M} \mathrm{HCl}\), (c) \(0.70 \mathrm{M} \mathrm{KOH}\) (d) \(0.40 \mathrm{M} \mathrm{NaNO}_{3}\).

Calculate the \(\mathrm{pH}\) of a \(0.42 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\) solution.

\(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a strong acid, but \(\mathrm{HSO}_{4}^{-}\) is a weak acid. Account for the difference in strength of these two related species.
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