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:**
What is the hydroxide ion concentration for a 23 % (m/v) HNO₃ solution?
**Explanation:**
The question asks for the concentration of hydroxide ions (OH⁻) in a solution containing 23% (mass/volume) nitric acid (HNO₃). Here’s a step-by-step guide to approach this problem:
1. **Understand the nature of HNO₃:**
- Nitric acid (HNO₃) is a strong acid which dissociates completely in water. The dissociation reaction is:
\[ \text{HNO}_3 \rightarrow \text{H}^+ + \text{NO}_3^- \]
2. **Calculate the concentration of H⁺ ions:**
- Since HNO₃ is a strong acid, the concentration of H⁺ ions ([H⁺]) will be approximately equal to the concentration of HNO₃.
3. **Use the relationship between H⁺ and OH⁻ concentrations:**
- The product of the concentrations of H⁺ and OH⁻ ions in water is always \( 1.0 \times 10^{-14} \) at 25°C (Kw value).
\[ \text{[H}^+][\text{OH}^-] = 1.0 \times 10^{-14} \]
4. **Determine the concentration of HNO₃ in molarity (M):**
- 23% (m/v) means 23 grams of HNO₃ per 100 mL solution.
- Molar mass of HNO₃ is approximately \(63 \, \text{g/mol}\).
- Calculate the molarity:
\[ \text{Molarity (M) of HNO}_3 = \frac{23 \, \text{g}}{63 \, \text{g/mol}} \times \frac{1}{0.100 \, \text{L}} \]
5. **Calculate the [OH⁻]:**
- Once [H⁺] is known, use the ion product of water to find [OH⁻]:
\[ \text{ [OH}^-] = \frac{1.0 \times 10^{-14}}{\text{ [H}^+]} \]
**Note:** If specific](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa9e8573f-552b-4431-b931-fec80f931989%2F710cffad-8e0a-4e52-b077-2442439d6dc6%2Fz0hoiyi_processed.png&w=3840&q=75)
Transcribed Image Text:**Question:**
What is the hydroxide ion concentration for a 23 % (m/v) HNO₃ solution?
**Explanation:**
The question asks for the concentration of hydroxide ions (OH⁻) in a solution containing 23% (mass/volume) nitric acid (HNO₃). Here’s a step-by-step guide to approach this problem:
1. **Understand the nature of HNO₃:**
- Nitric acid (HNO₃) is a strong acid which dissociates completely in water. The dissociation reaction is:
\[ \text{HNO}_3 \rightarrow \text{H}^+ + \text{NO}_3^- \]
2. **Calculate the concentration of H⁺ ions:**
- Since HNO₃ is a strong acid, the concentration of H⁺ ions ([H⁺]) will be approximately equal to the concentration of HNO₃.
3. **Use the relationship between H⁺ and OH⁻ concentrations:**
- The product of the concentrations of H⁺ and OH⁻ ions in water is always \( 1.0 \times 10^{-14} \) at 25°C (Kw value).
\[ \text{[H}^+][\text{OH}^-] = 1.0 \times 10^{-14} \]
4. **Determine the concentration of HNO₃ in molarity (M):**
- 23% (m/v) means 23 grams of HNO₃ per 100 mL solution.
- Molar mass of HNO₃ is approximately \(63 \, \text{g/mol}\).
- Calculate the molarity:
\[ \text{Molarity (M) of HNO}_3 = \frac{23 \, \text{g}}{63 \, \text{g/mol}} \times \frac{1}{0.100 \, \text{L}} \]
5. **Calculate the [OH⁻]:**
- Once [H⁺] is known, use the ion product of water to find [OH⁻]:
\[ \text{ [OH}^-] = \frac{1.0 \times 10^{-14}}{\text{ [H}^+]} \]
**Note:** If specific
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