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Determine the H*|, pH, and pOH of a solution with an OH-] of 4.2 x 10-12 M at 25 °C. [H*] = M %3D pH = pOH = Determine the H*], OH-, and pOH of a solution with a pH of 10.33 at 25 °C.

Determine the H*|, pH, and pOH of a solution with an OH-] of 4.2 x 10-12 M at 25 °C. [H*] = M %3D pH = pOH = Determine the H*], OH-, and pOH of a solution with a pH of 10.33 at 25 °C.

Chemistry
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
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**Chemistry Calculations: Understanding pH and pOH** 1. **Determine the \([H^+]\), pH, and pOH of a solution with an \([OH^-]\) of \(4.2 \times 10^{-12}\) M at 25°C.** - \([H^+]\) = __________ M - pH = __________ - pOH = __________ 2. **Determine the \([H^+]\), \([OH^-]\), and pOH of a solution with a pH of 10.33 at 25°C.** **Instructions:** To solve these problems, use the following formulas and relationships: - \([H^+]\) and \([OH^-]\) are related by the ion product of water: \([H^+][OH^-] = 1.0 \times 10^{-14}\) at 25°C. - The pH is calculated as: \( \text{pH} = -\log[H^+]\) - The pOH is calculated as: \( \text{pOH} = -\log[OH^-]\) - The relationship between pH and pOH is: \( \text{pH} + \text{pOH} = 14\) Fill in the blanks with the appropriate values calculated using these relationships.
Transcribed Image Text:**Chemistry Calculations: Understanding pH and pOH** 1. **Determine the \([H^+]\), pH, and pOH of a solution with an \([OH^-]\) of \(4.2 \times 10^{-12}\) M at 25°C.** - \([H^+]\) = __________ M - pH = __________ - pOH = __________ 2. **Determine the \([H^+]\), \([OH^-]\), and pOH of a solution with a pH of 10.33 at 25°C.** **Instructions:** To solve these problems, use the following formulas and relationships: - \([H^+]\) and \([OH^-]\) are related by the ion product of water: \([H^+][OH^-] = 1.0 \times 10^{-14}\) at 25°C. - The pH is calculated as: \( \text{pH} = -\log[H^+]\) - The pOH is calculated as: \( \text{pOH} = -\log[OH^-]\) - The relationship between pH and pOH is: \( \text{pH} + \text{pOH} = 14\) Fill in the blanks with the appropriate values calculated using these relationships.
**Exercise: Calculating pH, pOH, and Ion Concentrations** **Problem 1:** Determine the \([OH^-]\), pH, and pOH of a solution with a \([H^+]\) of \(5.9 \times 10^{-6}\) M at 25 °C. - \([OH^-]\) = \_\_\_\_\_\_\_\_ M - pH = \_\_\_\_\_\_\_\_ - pOH = \_\_\_\_\_\_\_\_ --- **Problem 2:** Determine the \([H^+]\), pH, and pOH of a solution with an \([OH^-]\) of \(4.2 \times 10^{-12}\) M at 25 °C. - \([H^+]\) = \_\_\_\_\_\_\_\_ M - pH = \_\_\_\_\_\_\_\_ - pOH = \_\_\_\_\_\_\_\_ --- **Guidance for Solutions:** - To find \([OH^-]\) when \([H^+]\) is known, use the relationship: \[ [H^+] \times [OH^-] = 1.0 \times 10^{-14} \, \text{at 25 °C} \] - To calculate pH, use: \[ \text{pH} = -\log[H^+] \] - For pOH, the formula is: \[ \text{pOH} = -\log[OH^-] \] - Remember: \[ \text{pH} + \text{pOH} = 14 \, \text{at 25 °C} \] Use these formulas to fill in the blanks and determine the required values.
Transcribed Image Text:**Exercise: Calculating pH, pOH, and Ion Concentrations** **Problem 1:** Determine the \([OH^-]\), pH, and pOH of a solution with a \([H^+]\) of \(5.9 \times 10^{-6}\) M at 25 °C. - \([OH^-]\) = \_\_\_\_\_\_\_\_ M - pH = \_\_\_\_\_\_\_\_ - pOH = \_\_\_\_\_\_\_\_ --- **Problem 2:** Determine the \([H^+]\), pH, and pOH of a solution with an \([OH^-]\) of \(4.2 \times 10^{-12}\) M at 25 °C. - \([H^+]\) = \_\_\_\_\_\_\_\_ M - pH = \_\_\_\_\_\_\_\_ - pOH = \_\_\_\_\_\_\_\_ --- **Guidance for Solutions:** - To find \([OH^-]\) when \([H^+]\) is known, use the relationship: \[ [H^+] \times [OH^-] = 1.0 \times 10^{-14} \, \text{at 25 °C} \] - To calculate pH, use: \[ \text{pH} = -\log[H^+] \] - For pOH, the formula is: \[ \text{pOH} = -\log[OH^-] \] - Remember: \[ \text{pH} + \text{pOH} = 14 \, \text{at 25 °C} \] Use these formulas to fill in the blanks and determine the required values.
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