### Example Question on pH and Hydrogen Ion Concentration:**30. Calculate the \([ \text{H}^+ ]\) in a solution that has a pH of 7.0.****Given Choices:**a. \( 3.9 \, M \)b. \( 10.1 \, M \)c. \( 1.2 \times 10^{-4} \, M \)d. \( 1.0 \times 10^{-7} \, M \)#### Explanation:To find the hydrogen ion concentration \([ \text{H}^+ ]\), we can use the relationship between pH and \([ \text{H}^+ ]\):\[ \text{pH} = -\log [ \text{H}^+ ] \]For a solution with a pH of 7.0,\[ 7.0 = -\log [ \text{H}^+ ] \]Rewriting this equation to solve for \([ \text{H}^+ ]\):\[ [ \text{H}^+ ] = 10^{-7} \, M \]Since the pH is neutral (pH = 7.0), the hydrogen ion concentration is:\[ [ \text{H}^+ ] = 1.0 \times 10^{-7} \, M \]Thus, the correct answer is:d. \( 1.0 \times 10^{-7} \, M \)

pH => We know that pH is calculate in 0 -14 range If the resultant or final pH value for a…

Answered: 30. Calculate the [H*] in a solution…

30. Calculate the [H*] in a solution that has a pH of 7.0. a. 3.9 M b. 10.1 M c. 1.2 x 104 M d. 1.0 x 10-7M 2482000-2004) all skols 15--100=10 =419-215

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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It’s all one chart, it just didn’t fit.