**A solution with pOH = 11.0.**\[ \text{[H}^+\text{]} = \underline{\hspace{6cm}} \, \text{M} \]*Explanation:*This text provides information about a solution with a given pOH value, which is 11.0. It prompts the reader to determine the concentration of hydrogen ions \([\text{H}^+]\) and provides a blank space for the answer in molarity (M). To calculate \([\text{H}^+]\), one can use the relationship between pH and pOH in aqueous solutions: \[\text{pH} + \text{pOH} = 14\]First, calculate the pH:\[\text{pH} = 14 - \text{pOH} = 14 - 11.0 = 3.0\]Then, use the formula:\[[\text{H}^+] = 10^{-\text{pH}} = 10^{-3.0} = 0.001 \, \text{M}\]The resulting concentration of hydrogen ions \([\text{H}^+]\) is therefore 0.001 M. **Determine the concentration of H\(^+\) in each solution at 25 °C.****A solution with pH = 1.0.**\[ \text{[H}^+\text{]} = \] \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ M**A solution with pH = 6.0.**\[ \text{[H}^+\text{]} = \] \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ M

For any solution: pH+ pOH = 14 Now, if pOH= 11.0 Then, pH = 14-11.0 = 3.0 Further, for any solution: pH= -log [H+] Hence, [H+] = 10-pH = 10-3 M Hence, concentration of [H+] =10-3 MHere, two solutions are given at 25⁰C. Solution (1) When, pH= 1.0, [H+] = 10-pH = 10-1.0 M = 0.1 M Hence, concentration of [H+] =0.1 M Solution (2) When, pH= 6.0, [H+] = 10-pH = 10-6.0 M = 10-6 M Hence, concentration of [H+] =10-6 M

Answered: A solution with pOH 11.0. %3D [H*] = M…

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Chemistry

A solution with pOH 11.0. %3D [H*] = M %3D

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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