Ch.16 - Acid-Base Equilibria

Problem 99d

Chapter 16, Problem 99d

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.

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Understand the nature of the K+ ion: Potassium ion (K+) is a cation formed when potassium loses one electron.

Consider the concept of acidity in water: A species is considered acidic if it can donate a proton (H+) to water, increasing the concentration of H3O+ ions.

Evaluate the interaction of K+ with water: K+ is a large, monovalent cation with a low charge density, meaning it does not significantly polarize water molecules.

Analyze the effect of K+ on water acidity: Since K+ does not polarize water molecules effectively, it does not increase the acidity of water by donating protons or causing water to release protons.

Conclude the statement's correctness: Based on the analysis, determine whether the statement about K+ ion being acidic in water is correct or incorrect.

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Key Concepts

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

Acidity and Basicity

Acidity refers to the ability of a substance to donate protons (H+) in a solution, while basicity refers to the ability to accept protons. In aqueous solutions, acids increase the concentration of H+ ions, which lowers the pH, making the solution more acidic. Understanding these definitions is crucial for evaluating the behavior of ions like K+ in water.

Hydration of Ions

When ions dissolve in water, they interact with water molecules, forming a hydration shell. This process can influence the properties of the solution, including its acidity. However, the K+ ion, being a cation of a strong base (KOH), does not significantly affect the pH of water, as it does not lead to an increase in H+ concentration.

Strong vs. Weak Acids and Bases

Strong acids and bases completely dissociate in water, while weak acids and bases do not. The K+ ion originates from potassium hydroxide, a strong base, which means it does not contribute to acidity in solution. Recognizing the strength of acids and bases is essential for determining the behavior of ions in aqueous environments.

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Strong vs Weak Bases

Related Practice

Textbook Question

Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true. (a) In general, the acidity of binary acids increases from left to right in a given row of the periodic table. (b) In a series of acids that have the same central atom, acid strength increases with the number of hydrogen atoms bonded to the central atom. (c) Hydrotelluric acid 1H2Te2 is a stronger acid than H2S because Te is more electronegative than S.

Textbook Question

Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true. (a) Acid strength in a series of H¬A molecules increases with increasing size of A. (b) For acids of the same general structure but differing electronegativities of the central atoms, acid strength decreases with increasing electronegativity of the central atom. (c) The strongest acid known is HF because fluorine is the most electronegative element.

Textbook Question

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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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

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.

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

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.

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Key Concepts

Acidity and Basicity

Hydration of Ions

Strong vs. Weak Acids and Bases

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.