Textbook Question
Determine whether each anion is basic or neutral. For those anions that are basic, write an equation that shows how the anion acts as a base. c. NO3–
Ch.17 - Acids and Bases
Chapter 17, Problem 99a
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. a. NH4+
Verified step by step guidance1
Identify the cation in question: \( \text{NH}_4^+ \).
Recall that a cation can be acidic if it can donate a proton (\( \text{H}^+ \)) to water, forming \( \text{H}_3\text{O}^+ \).
Consider the nature of \( \text{NH}_4^+ \): it is the conjugate acid of \( \text{NH}_3 \), a weak base.
Since \( \text{NH}_4^+ \) can donate a proton to water, it is considered acidic.
Write the chemical equation showing \( \text{NH}_4^+ \) acting as an acid: \( \text{NH}_4^+ + \text{H}_2\text{O} \rightarrow \text{NH}_3 + \text{H}_3\text{O}^+ \).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acidic Cations
Acidic cations are positively charged ions that can donate protons (H+) in solution, thereby lowering the pH. These cations typically come from weak bases or are derived from the hydrolysis of metal ions. Understanding whether a cation is acidic involves recognizing its ability to interact with water and produce H+ ions.
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pH and Acidity
pH is a measure of the hydrogen ion concentration in a solution, indicating its acidity or basicity. A pH less than 7 is considered acidic, while a pH of 7 is neutral. The relationship between cations and pH is crucial for determining whether a cation will affect the acidity of a solution.
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Hydrolysis Reactions
Hydrolysis reactions involve the reaction of a cation with water, leading to the formation of an acid and hydroxide ions. For example, when NH4+ (ammonium ion) is dissolved in water, it can donate a proton to water, forming NH3 (ammonia) and H3O+ (hydronium ion), thus demonstrating its acidic nature.
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Related Practice
Textbook Question
Determine the [OH–] and pH of a solution that is 0.140 M in F–.
Textbook Question
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. b. Na+
Textbook Question
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. c. Co3+
Textbook Question
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. d. CH2NH3+