**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

The ratio of moles to the volume of solution in liters is known as molarity.

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Chemistry

What is the hydroxide ion concentration for a 23 % (m/v) HNO3 solution?

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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