Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
Write an equation to show that hydrocyanic acid , HCN , behaves as an acid in water.
![**Title: Understanding the Acid Behavior of Hydrocyanic Acid (HCN) in Water**
**Equation Context:**
To demonstrate how hydrocyanic acid (HCN) acts as an acid when dissolved in water, we need to understand the basic reaction that occurs. Acids are substances that donate protons (H⁺ ions) to other entities.
**Chemical Equation:**
\[ \text{HCN} + \text{H}_2\text{O} \leftrightarrows \text{H}_3\text{O}^+ + \text{CN}^- \]
**Explanation:**
1. **Reactants:**
- **HCN:** Hydrocyanic acid, the acid in this reaction.
- **H₂O:** Water, which acts as the base.
2. **Products:**
- **H₃O⁺ (Hydronium Ion):** Forms when HCN donates a proton (H⁺) to the water molecule.
- **CN⁻ (Cyanide Ion):** The conjugate base of HCN after losing a proton.
**Conceptual Understanding:**
In an aqueous solution, HCN donates a proton to the water. This proton transfer leads to the formation of the hydronium ion (H₃O⁺), which is indicative of the acidic nature of a solution, and the cyanide ion (CN⁻), demonstrating the acid's dissociation. This reaction is reversible and the equilibrium lies towards the reactants, indicating that HCN is a weak acid.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb41c431a-d537-4c9f-b640-b49be1be5173%2Fa9504f24-edb0-469a-96be-0a04e23014e4%2Fmv0qp54_processed.png&w=3840&q=75)
Transcribed Image Text:**Title: Understanding the Acid Behavior of Hydrocyanic Acid (HCN) in Water**
**Equation Context:**
To demonstrate how hydrocyanic acid (HCN) acts as an acid when dissolved in water, we need to understand the basic reaction that occurs. Acids are substances that donate protons (H⁺ ions) to other entities.
**Chemical Equation:**
\[ \text{HCN} + \text{H}_2\text{O} \leftrightarrows \text{H}_3\text{O}^+ + \text{CN}^- \]
**Explanation:**
1. **Reactants:**
- **HCN:** Hydrocyanic acid, the acid in this reaction.
- **H₂O:** Water, which acts as the base.
2. **Products:**
- **H₃O⁺ (Hydronium Ion):** Forms when HCN donates a proton (H⁺) to the water molecule.
- **CN⁻ (Cyanide Ion):** The conjugate base of HCN after losing a proton.
**Conceptual Understanding:**
In an aqueous solution, HCN donates a proton to the water. This proton transfer leads to the formation of the hydronium ion (H₃O⁺), which is indicative of the acidic nature of a solution, and the cyanide ion (CN⁻), demonstrating the acid's dissociation. This reaction is reversible and the equilibrium lies towards the reactants, indicating that HCN is a weak acid.
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