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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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
Transcribed Image Text:Calculate the pH of 1.00 L of the buffer
Part 1 of 3
Note: Reference the pK of acids at 25 °C table for additional information.
a
4.73
pH of starting buffer: Be sure your answer has the correct number of significant digits.
Part 2 of 3
×...
4.76
Part 3 of 3
x10
×
pH after addition of 0.040 mol NaOH: Be sure your answer has the correct number of significant digits.
4.61
x10
X
Ś
x10
0.99 M CH3COONa
1.02 M CH₂COOH
X
before and after the addition of the following species. (Assume there is no change in volume.)
Ś
pH after further addition of 0.133 mol HCl: Be sure your answer has the correct number of significant digits.
Ś
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- A 1.451.45 L buffer solution consists of 0.1590.159 M butanoic acid and 0.3320.332 M sodium butanoate. Calculate the pH of the solution following the addition of 0.0620.062 moles of NaOHNaOH. Assume that any contribution of the NaOHNaOH to the volume of the solution is negligible. The ?aKa of butanoic acid is 1.52×10−51.52×10−5.arrow_forwardWhat is the pH of a buffer that contains 0.356 M H2C6H606 and 0.647 М НС,Н,О6? Ka1 = 7.9 × 10-5 Ka2 = 1.6 x 10-12 IMPORTANT: When entering your answer: • Erter the number only (no units) • Do not leave any spaces • Use a leading zero before the decimal when necessary Report your number to 2 decimal places (regardless of the significant figures) • Correctly round your answer to the 2nd decimal place (allowed margin of error is only + 0.01, so always use un- rounded numbers in your calculations) Examples: 0.12 or 9.87arrow_forwardPlease don't provide handwritten solution... A 1.0 L solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value for Ka HC2H3O2 is 1.8 X 10-5. What is the pH of the buffer after adding 0.010 mol NaOH to the buffer.arrow_forward
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- A 10.0mL solution of 0.720 M NH3 is titrated with a 0.240 M HCl solution. Calculate the pH after the following additions of the HCl solution: 0.00mL, 10.0mL, 30.0mL, and 40.0mL. Be sure your answer has the correct number of significant digits. 0.00 mL added, pH = 10.0 mL added, pH = 30.0 mL added, pH = 40.0 mL added, pH =arrow_forwardPart 3: pH after addition of 0.145mol HCl: Round your answer to 2 decimal placesarrow_forwardA chemist titrates 90.0 mL of a 0.2182M acetic acid (HCH3CO₂) solution with 0.8569M NaOH solution at 25 °C. Calculate the pH at equivalence. The p K of acetic acid is 4.76. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NaOH solution added. pH = 0 X 3 ?arrow_forward
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