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Ch.16 - Acid-Base Equilibria
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.16 - Acid-Base EquilibriaProblem 99c
Chapter 16, Problem 99c

Indicate whether each of the following statements is correct or incorrect. (c) Conjugate acids of weak bases produce more acidic solutions than conjugate acids of strong bases.

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1
Identify the concept of conjugate acids and bases. A conjugate acid is formed when a base gains a proton (H⁺).
Understand the relationship between the strength of a base and its conjugate acid. The weaker the base, the stronger its conjugate acid.
Recall that weak bases have stronger conjugate acids compared to strong bases, which have weaker conjugate acids.
Consider the effect of a strong conjugate acid in solution. Stronger conjugate acids will donate protons more readily, making the solution more acidic.
Conclude that the statement is correct: conjugate acids of weak bases produce more acidic solutions than conjugate acids of strong bases.

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Key Concepts

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

Conjugate Acid-Base Pairs

In acid-base chemistry, a conjugate acid is formed when a base accepts a proton (H+). The strength of the conjugate acid depends on the strength of the original base; weak bases yield stronger conjugate acids, while strong bases yield weaker conjugate acids. This relationship is crucial for understanding the acidity of solutions formed from these pairs.

Strength of Acids and Bases

Acids and bases are classified as strong or weak based on their ability to dissociate in water. Strong acids completely dissociate, while weak acids only partially dissociate. This distinction affects the pH of the resulting solutions, with weak acids contributing to a higher pH compared to strong acids, which produce lower pH values.
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Strength of Conjugate Acids and Bases

pH and Solution Acidity

pH is a measure of the hydrogen ion concentration in a solution, indicating its acidity or basicity. A lower pH value corresponds to a more acidic solution. Understanding how conjugate acids influence pH is essential for evaluating the acidity of solutions derived from weak and strong bases, as the nature of the conjugate acid directly impacts the solution's pH.
Related Practice
Textbook Question

Which, if any, of the following statements are true? (a) The stronger the base, the smaller the pKb. (b) The stronger the base, the larger the pKb. (c) The stronger the base, the smaller the Kb. (d) The stronger the base, the larger the Kb. (e) The stronger the base, the smaller the pKa of its conjugate acid. (f) The stronger the base, the larger the pKa of its conjugate acid.

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Textbook Question

Predict how each molecule or ion would act, in the Brønsted-Lowry sense, in aqueous solution by writing 'acid,' 'base,' 'both,' or 'neither' on the line provided. (b) Prozac

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Textbook Question

Identify the Lewis acid and Lewis base among the reactants in each of the following reactions:

(a) Fe(ClO4)3(s) + 6 H2O(l) ⇌ [Fe(H2O)6]3+(aq) + 3 ClO4-(aq)

(b) CN-(aq) + H2O(l) ⇌ HCN(aq) + OH-(aq)

(c) (CH3)3N(g) + BF3(g) ⇌ (CH3)NBF3(s)

(d) HIO(lq) + NH2-(lq) ⇌ NH3(lq) + IO-(lq) (lq denotes liquid ammonia as solvent)

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Textbook Question

Identify the Lewis acid and Lewis base in each of the following reactions:

(a) HNO2(aq) + OH-(aq) ⇌ NO2-(aq) + H2O(l)

(b) FeBr3(s) + Br-(aq) ⇌ FeBr4-(aq)

(c) Zn2+(aq) + 4 NH3(aq) ⇌ Zn(NH3)42+(aq)

(d) SO2(g) + H2O(l) ⇌ H2SO3(aq)

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Textbook Question

A solution is made by adding 0.300 g Ca1OH221s2, 50.0 mL of 1.40 M HNO3, and enough water to make a final volume of 75.0 mL. Assuming that all of the solid dissolves, what is the pH of the final solution?

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