Temperature-Dependence of Kw: The autoionization of water is an endothermic reaction. According to the Le Châtelier's Principle, adding heat will favor the formation of H30*and OH¯. As a result, the value of Kw will increase with increasing temperature, and the pH will decrease with increasing temperature. Complete the following table to determine Kw, [H30*], and pH for pure water at different temperatures. Temperature (C) Kw [H30*] pH 0.0°C 1.14 x 10-15 3.38 x 10-8 M 7.47 10.0 °C 2.93 x 10-15 20.0 °C 8.25 x 10-8 M 30.0 °C 1.47 x 10-14 37.0 °C 6.81 40.0 °C 1.71 x 10-7 M 6.63 50.0 °C Show your work:
Temperature-Dependence of Kw: The autoionization of water is an endothermic reaction. According to the Le Châtelier's Principle, adding heat will favor the formation of H30*and OH¯. As a result, the value of Kw will increase with increasing temperature, and the pH will decrease with increasing temperature. Complete the following table to determine Kw, [H30*], and pH for pure water at different temperatures. Temperature (C) Kw [H30*] pH 0.0°C 1.14 x 10-15 3.38 x 10-8 M 7.47 10.0 °C 2.93 x 10-15 20.0 °C 8.25 x 10-8 M 30.0 °C 1.47 x 10-14 37.0 °C 6.81 40.0 °C 1.71 x 10-7 M 6.63 50.0 °C Show your work:
Chemistry
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Chapter1: Chemical Foundations
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![**Temperature-Dependence of \( K_w \):**
The autoionization of water is an endothermic reaction. According to Le Châtelier’s Principle, adding heat will favor the formation of \( H_3O^+ \) and \( OH^- \). As a result, the value of \( K_w \) will increase with increasing temperature, and the pH will decrease with increasing temperature.
Complete the following table to determine \( K_w \), \( [H_3O^+] \), and pH for pure water at different temperatures.
| Temperature (°C) | \( K_w \) | \( [H_3O^+] \) | pH |
|------------------|----------------------|----------------------|-----|
| 0.0 °C | \( 1.14 \times 10^{-15} \) | \( 3.38 \times 10^{-8} \, \text{M} \) | 7.47 |
| 10.0 °C | \( 2.93 \times 10^{-15} \) | | |
| 20.0 °C | | \( 8.25 \times 10^{-8} \, \text{M} \) | |
| 30.0 °C | \( 1.47 \times 10^{-14} \) | | |
| 37.0 °C | | | 6.81 |
| 40.0 °C | | \( 1.71 \times 10^{-7} \, \text{M} \) | |
| 50.0 °C | | | 6.63 |
**Show your work:**
*(Note: The section reserved for showing work is blank, awaiting student input or calculations.)*
This table illustrates the relationship between temperature and the equilibrium constant \( K_w \), the concentration of hydronium ions \( [H_3O^+] \), and the pH of pure water.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fea7914d9-9db2-49c2-97e0-da9d8983400b%2F0d4a992c-f676-4acc-8308-1be89ff4f365%2Fnlpumd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Temperature-Dependence of \( K_w \):**
The autoionization of water is an endothermic reaction. According to Le Châtelier’s Principle, adding heat will favor the formation of \( H_3O^+ \) and \( OH^- \). As a result, the value of \( K_w \) will increase with increasing temperature, and the pH will decrease with increasing temperature.
Complete the following table to determine \( K_w \), \( [H_3O^+] \), and pH for pure water at different temperatures.
| Temperature (°C) | \( K_w \) | \( [H_3O^+] \) | pH |
|------------------|----------------------|----------------------|-----|
| 0.0 °C | \( 1.14 \times 10^{-15} \) | \( 3.38 \times 10^{-8} \, \text{M} \) | 7.47 |
| 10.0 °C | \( 2.93 \times 10^{-15} \) | | |
| 20.0 °C | | \( 8.25 \times 10^{-8} \, \text{M} \) | |
| 30.0 °C | \( 1.47 \times 10^{-14} \) | | |
| 37.0 °C | | | 6.81 |
| 40.0 °C | | \( 1.71 \times 10^{-7} \, \text{M} \) | |
| 50.0 °C | | | 6.63 |
**Show your work:**
*(Note: The section reserved for showing work is blank, awaiting student input or calculations.)*
This table illustrates the relationship between temperature and the equilibrium constant \( K_w \), the concentration of hydronium ions \( [H_3O^+] \), and the pH of pure water.
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