Answered: 9.16×10-2 M HCIO, Express your answer…

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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$The image displays a section from an online chemistry educational platform where students are prompted to calculate the pH of a given solution. Below is a detailed transcription and explanation: --- **Part B** Given concentration: $ 9.16 \times 10^{-2} \, M \, \text{HClO}_4 $ Prompt: Express your answer to three decimal places. **Input Field:** - A text box labeled "pH = " where students enter their calculated pH value. **Controls and Buttons:** - A set of icons for input options (such as a calculator or Greek symbols). - A “Submit” button followed by a “Request Answer” option. There are also notes for completing preceding parts: - **Part C**: Complete previous part(s) - **Part D**: Complete previous part(s) **Page Footer:** - Pearson logo and copyright information. - Links to Terms of Use, Privacy Policy, Permissions, and Contact Us. **Explanation:** The exercise instructs students to calculate the pH of a 0.0916 M perchloric acid ($\text{HClO}_4$) solution. Given that $\text{HClO}_4$ is a strong acid, it dissociates completely in solution. Thus, the concentration of hydronium ions ($[H_3O^+]$) is equal to the initial concentration of the acid. The pH is calculated using the formula: \[ \text{pH} = -\log[H_3O^+] \] Students must perform this calculation and input the pH value to three decimal places in the provided text box. --- This structure ensures students understand how to approach calculating pH for strong acids and reinforces the use of logarithmic functions in chemistry.$

Transcribed Image Text:The image displays a section from an online chemistry educational platform where students are prompted to calculate the pH of a given solution. Below is a detailed transcription and explanation: --- **Part B** Given concentration: $ 9.16 \times 10^{-2} \, M \, \text{HClO}_4 $ Prompt: Express your answer to three decimal places. **Input Field:** - A text box labeled "pH = " where students enter their calculated pH value. **Controls and Buttons:** - A set of icons for input options (such as a calculator or Greek symbols). - A “Submit” button followed by a “Request Answer” option. There are also notes for completing preceding parts: - **Part C**: Complete previous part(s) - **Part D**: Complete previous part(s) **Page Footer:** - Pearson logo and copyright information. - Links to Terms of Use, Privacy Policy, Permissions, and Contact Us. **Explanation:** The exercise instructs students to calculate the pH of a 0.0916 M perchloric acid ($\text{HClO}_4$) solution. Given that $\text{HClO}_4$ is a strong acid, it dissociates completely in solution. Thus, the concentration of hydronium ions ($[H_3O^+]$) is equal to the initial concentration of the acid. The pH is calculated using the formula: \[ \text{pH} = -\log[H_3O^+] \] Students must perform this calculation and input the pH value to three decimal places in the provided text box. --- This structure ensures students understand how to approach calculating pH for strong acids and reinforces the use of logarithmic functions in chemistry.

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