Please help with part C ### pH of a Strong Acid and a Strong Base**pH Definition:**pH is a logarithmic scale used to indicate the hydrogen ion concentration, \([H^+]\), of a solution:\[ \text{pH} = -\log[H^+] \]**Relationship Between pH and pOH:**Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, \([OH^-]\), are related to each other by the ion product constant of water, \(K_w\):\[ K_w = [H^+][OH^-] = 1.00 \times 10^{-14} \]Here, \(1.00 \times 10^{-14}\) is the value at approximately 297 K. Based on this relationship, pH and pOH are related as follows:\[ 14.00 = \text{pH} + \text{pOH} \]---**Part B: Calculating pH**0.90 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 8.0 L of solution. To find the pH of this solution, express the pH numerically to two decimal places. The calculated pH is:\[ \text{pH} = 11.45 \]The answer is marked as correct with a note explaining that because the concentration had two significant figures, the pH has two digits after the decimal point.---**Part C: Calculating pOH**Given the solution in Part B, calculate the pOH. Express the pOH numerically to two decimal places. Input the calculated pOH in the provided field.--- This educational page outlines the fundamental relationships between pH, pOH, and the concentration of ions in a solution, using the example of sodium hydroxide to illustrate calculation methods.

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pH is a logarithmic scale used to indicate the hydrogen ion concentration, [H], of a solution: pH = -log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH-], are related to each other by the K of water: K = [H+][OH-] = 1.00 × 10-¹4 where 1.00 x 10-14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00 pH + pOH Submit ✔ Correct Because the concentration had two significant figures, the pH has two digits after the decimal point. Part B 0.90 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 8.0 L of solution. What is the pH of this solum Express the pH numerically to two decimal places. View Available Hint(s) pH = 11.45 Buben't Previous Answers Part C ✓ Correct Because the concentration had two significant figures, the pH has two digits after the decimal point. POH = Previous Answers What is the pOH of the solution in Part B? Express the pOH numerically to two decimal places. Submit VG ΑΣΦ Request Answer ?

pH is a logarithmic scale used to indicate the hydrogen ion concentration, [H], of a solution: pH = -log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH-], are related to each other by the K of water: K = [H+][OH-] = 1.00 × 10-¹4 where 1.00 x 10-14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00 pH + pOH Submit ✔ Correct Because the concentration had two significant figures, the pH has two digits after the decimal point. Part B 0.90 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 8.0 L of solution. What is the pH of this solum Express the pH numerically to two decimal places. View Available Hint(s) pH = 11.45 Buben't Previous Answers Part C ✓ Correct Because the concentration had two significant figures, the pH has two digits after the decimal point. POH = Previous Answers What is the pOH of the solution in Part B? Express the pOH numerically to two decimal places. Submit VG ΑΣΦ Request 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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