MISSED THIS? Read Section 17.9. You can click on the Review link to access the section in your eText. Calculate [H3O+] and the pH of each H2SO4 solution (Ka2 =0.012). At approximately what concentration does the x is small approximation break down? Part B Calculate the pH of a 0.54 M solution. Express your answer to two decimal places. ■ ΑΣΦ pH = 1.1 Submit Previous Answers Request Answer ? × Incorrect; Try Again; 8 attempts remaining To determine the pH of the solution, substitute the value of [H3O+] calculated in Part A into the equation that defines pH: ▾ Part C pH = -log[H3O+] Calculate [H3O+] for a 0.18 M solution. Express your answer in molarity to two significant figures. ΜΕ ΑΣΦ [H3O+]= Submit Request Answer ? M
MISSED THIS? Read Section 17.9. You can click on the Review link to access the section in your eText. Calculate [H3O+] and the pH of each H2SO4 solution (Ka2 =0.012). At approximately what concentration does the x is small approximation break down? Part B Calculate the pH of a 0.54 M solution. Express your answer to two decimal places. ■ ΑΣΦ pH = 1.1 Submit Previous Answers Request Answer ? × Incorrect; Try Again; 8 attempts remaining To determine the pH of the solution, substitute the value of [H3O+] calculated in Part A into the equation that defines pH: ▾ Part C pH = -log[H3O+] Calculate [H3O+] for a 0.18 M solution. Express your answer in molarity to two significant figures. ΜΕ ΑΣΦ [H3O+]= Submit Request Answer ? M
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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