Use the acid-dissociation constants in Table 16.3 to arrange these oxyanions from strongest base to weakest: SO42-, CO32-, SO32-, and PO43-.

Verified step by step guidance

Identify the conjugate acids of each oxyanion: HSO4- for SO42-, HCO3- for CO32-, HSO3- for SO32-, and HPO4^2- for PO43-.

Refer to Table 16.3 to find the acid-dissociation constants (Ka) for each conjugate acid. Remember, a lower Ka value indicates a weaker acid.

Understand that the strength of the base (oxyanion) is inversely related to the strength of its conjugate acid. Thus, the weaker the conjugate acid, the stronger the base.

Arrange the conjugate acids in order of increasing Ka values. This order will be the reverse for the oxyanions, from strongest base to weakest base.

List the oxyanions in the order derived from the previous step, starting with the one whose conjugate acid has the lowest Ka (strongest base) to the one with the highest Ka (weakest base).

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acid-Dissociation Constants (Ka)

Acid-dissociation constants (Ka) quantify the strength of an acid in solution, indicating how well it donates protons (H+) to water. A higher Ka value corresponds to a stronger acid, which means it dissociates more completely in solution. Understanding Ka is essential for comparing the basicity of oxyanions, as the conjugate bases of stronger acids are weaker bases.

Oxyanions and Their Basicity

Oxyanions are negatively charged ions that contain oxygen, and their basicity is influenced by the central atom and the number of oxygen atoms. Generally, the more electronegative the central atom or the more oxygen atoms present, the weaker the base. This is due to the stabilization of the negative charge by resonance and the ability of the central atom to withdraw electron density.

Comparative Analysis of Oxyanions

To arrange oxyanions from strongest to weakest base, one must compare their acid-dissociation constants and the stability of their conjugate acids. By analyzing the Ka values of the corresponding acids, one can infer the relative strength of the oxyanions as bases. This comparative analysis is crucial for determining the order of basicity among the given oxyanions.

Recommended video:

Guided course

06:11

Dimensional Analysis

Related Practice

Textbook Question

Calculate Kb values for CH3COO- and ClO-.

views

Textbook Question

Which is the stronger base, the acetate ion or the hypochlorite ion?

Textbook Question

Ephedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base: C10H15ON1aq2 + H2O1l2 Δ C10H15ONH+1aq2 + OH-1aq2 A 0.035 M solution of ephedrine has a pH of 11.33. (b) Calculate Kb for ephedrine.

Textbook Question

Codeine 1C18H21NO32 is a weak organic base. A 5.0 * 10-3M solution of codeine has a pH of 9.95. Calculate the value of Kb for this substance. What is the pKb for this base?

Textbook Question

Given that Ka for acetic acid is 1.8 * 10-5 and that for hypochlorous acid is 3.0 * 10-8, which is the stronger acid?