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.

Verified step by step guidance

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.

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.

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.

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.

Recommended video:

Guided course

07:51

Calculating pH of Weak Acids Example

Related Practice

Textbook Question

Which member of each pair produces the more acidic aqueous solution: (a) ZnBr₂ or CdCl₂ (b) CuCl or Cu(NO₃)₂ (c) Ca(NO₃)₂ or NiBr₂

Textbook Question

Indicate whether each of the following statements is correct or incorrect. (d) K⁺ ion is acidic in water because it causes hydrating water molecules to become more acidic.

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?

Textbook Question

Salts containing the phosphate ion are added to municipal water supplies to prevent the corrosion of lead pipes. (a) Based on the pKa values for phosphoric acid 1pKa1 = 7.5 * 10 - 3, pKa2 = 6.2 * 10 - 8, pKa3 = 4.2 * 10 - 132 what is the Kb value for the PO43 - ion?