7. Refer to the following table:Table 2-2. Change in pH of 0.2 M Acetate Buffer after addition of Acid or Base[Base]:[Acid]0.005:0.195AdditionpHHC1 0.095 mol3.1HC1 0.0750.025:0.1753.9HС1 0.05НС1 0.0250.05:0.154.20.075:0.1254.50.1:0.10.125:0.0754.7NaOH 0.025 mol4.9NaOH 0.05 mol0.15:0.055.2NaOH 0.75 mol0.175:0.0255.5NaOH 0.095 mol0.195:0.0056.3a. Calculate the pH of a 0.2 M acetate buffer (a solution containing 0.1 mol L-' acetic acid and 0.1 mol L-1sodium acetate), given that the pKa of acetic acid is 4.7.b. What would be the pH value after adding 0.05 mol of NaOH to 1 L of 0.2 mol L1 acetate buffer?c. Compare the pH value in (b) with that obtained after adding 0.05 mol NAOH to 1 L of water (a simplesolution of 0.05 mol L-' NaOH).d. How much acid or base can be added to 1 L of the 0.2 M acetate buffer so that the pH does not changeappreciably (i.e., what is its buffer range)?

Answered: Image /qna-images/answer/cb8248a1-5a92-421a-9651-680d4361d207.jpg

a. Calculate the pH of a 0.2 M acetate buffer (a solution containing 0.1 mol L-l acetic acid and 0.1 mol L- sodium acetate), given that the pKa of acetic acid is 4.7. b. What would be the pH value after adding 0.05 mol of NaOH to 1 L of 0.2 mol L' acetate buffer? c. Compare the pH value in (b) with that obtained after adding 0.05 mol NaOH to 1 L of water (a simple solution of 0.05 mol L·1 NaOH).

a. Calculate the pH of a 0.2 M acetate buffer (a solution containing 0.1 mol L-l acetic acid and 0.1 mol L- sodium acetate), given that the pKa of acetic acid is 4.7. b. What would be the pH value after adding 0.05 mol of NaOH to 1 L of 0.2 mol L' acetate buffer? c. Compare the pH value in (b) with that obtained after adding 0.05 mol NaOH to 1 L of water (a simple solution of 0.05 mol L·1 NaOH).

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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Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HClO and 0.37 M NaClO. The value of Ka for HClO is 2.9 × 10⁻⁸. Determine the moles of the ractant and product after the reaction of the acid and base. (Similar to ICE format but is instead Before (mol), Change (mol), and After (mol) Determine the ICE table for HClO (aq) + H2O - H3O+ + ClO- (aq) Fill in Ka= ? = 2.9 * 10-8 Calculate pH
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24. How many moles of NH,Br must be added to 2 L of 0.1 M NH,OH to form a buffer whose pH is 9.00? (K, of NH,OH = 1.76 x 0*)
Consider a 1.0 L buffer containing 0.115 mol L HF and 0.105 mol L F. What is the pH of the solution after adding 1.9 x 103 mol of NaOH? Express your answer to 2 decimal places. Remember you can find K, and/or K, values in your textbook in chapter 15. They are also posted on eClass