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Chapter 16: Problem 37

What does the ionization constant tell us about the strength of an acid?

Short Answer

Expert verified
The ionization constant (Ka) tells us about the strength of an acid. A larger Ka denotes a stronger acid, as it indicates more extensive ionization and thus, greater production of H+ ions in a solution.

Step by step solution

01

Understanding Ionization Constant

The ionization constant of an acid, often termed the acid dissociation constant (Ka), is a measure of the strength of an acid in solution. It corresponds to the equilibrium between the acid (HA) and the ions produced when it dissociates. Therefore, in a simple HA 鈬� H+ + A- equilibrium, the ionization constant is typically written as Ka = [H+][A-] / [HA].
02

Significance of Ionization Constant

The ionization constant provides us with a quantitative measure of the degree to which the acid will ionize in a solution. The greater the Ka, the greater the extent of ionization, and hence, the greater the amount of hydrogen ions produced in the solution.
03

Relation with Strength of Acid

The strength of an acid is related to its ability to donate protons or hydrogen ions into solution. An acid with a larger ionization constant (Ka) will be a stronger acid, because it donates more H+ ions into the solution and therefore ionizes to a greater extent. Thus, the larger an acid's Ka, the stronger the acid.

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Most popular questions from this chapter

Prove the statement that when the concentration of a weak acid HA decreases by a factor of 10 , its percent ionization increases by a factor of \(\sqrt{10}\). State any assumptions.

What are the names and formulas of the conjugate bases of these acids: (a) \(\mathrm{HNO}_{2},\) (b) \(\mathrm{H}_{2} \mathrm{SO}_{4},\) (c) \(\mathrm{H}_{2} \mathrm{~S},\) (d) HCN, (e) HCOOH (formic acid)?

A 1.294 -g sample of a metal carbonate \(\left(\mathrm{MCO}_{3}\right)\) is reacted with \(500 \mathrm{~mL}\) of a \(0.100 \mathrm{M} \mathrm{HCl}\) solution. The excess \(\mathrm{HCl}\) acid is then neutralized by \(32.80 \mathrm{~mL}\) of \(0.588 M \mathrm{NaOH} .\) Identify M.

Consider the following compounds: Experimentally, phenol is found to be a stronger acid than methanol. Explain this difference in terms of the structures of the conjugate bases. (Hint: A more stable conjugate base favors ionization. Only one of the conjugate bases can be stabilized by resonance.

Write an equation relating \(\left[\mathrm{H}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) in solution at \(25^{\circ} \mathrm{C}\).
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