The buffer from Part A is diluted to 1.00 L. To half of it (500. mL), you add 0.0100 mol of hydrogen ions without changing the volume. What is the pH of the final solution? Express your answer numerically to two decimal places. ► View Available Hint(s) VE ΑΣΦ pH = 7.29 Submit Previous Answers X Incorrect; Try Again; 4 attempts remaining ?
The buffer from Part A is diluted to 1.00 L. To half of it (500. mL), you add 0.0100 mol of hydrogen ions without changing the volume. What is the pH of the final solution? Express your answer numerically to two decimal places. ► View Available Hint(s) VE ΑΣΦ pH = 7.29 Submit Previous Answers X Incorrect; Try Again; 4 attempts remaining ?
Chapter14: Principles Of Neutralization Titrations
Section: Chapter Questions
Problem 14.33QAP
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Transcribed Image Text:What volume of 10.0 M NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHCl?
Express your answer in milliliters using two significant figures.
► View Available Hint(s)
6.7 mL
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Correct
This procedure represents only one of many ways to prepare a buffer. The exact method chosen depends
on the reagents and glassware available as well as the accuracy required for the pH.
Transcribed Image Text:The buffer from Part A is diluted to 1.00 L. To half of it (500. mL), you add 0.0100 mol of hydrogen ions without
changing the volume. What is the pH of the final solution?
Express your answer numerically to two decimal places.
► View Available Hint(s)
VE ΑΣΦ
pH = 7.29
Submit
Previous Answers
X Incorrect; Try Again; 4 attempts remaining
?
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Step 1: Determine th pH of the final solution after add H+ ions:
VIEWStep 2: Calculation for moles of each species after add NaOH
VIEWStep 3: Calculation for moles of NaOH
VIEWStep 4: Calculation for moles of each species after add H+ ions:
VIEWStep 5: Calculation for final pH of the solution:
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