06 Question (1 point)See page 768LAUNCH TUTORIAL LESSONCOAST Tutorial ProblemConsider the following reaction:CH3COOH(aq) + OH(aq) CH₂COO¯(aq) + H2O(1)5th attemptSee HintHow much 5.80 M NaOH must be added to 520.0 mL of a buffer that is 0.0200 Macetic acid and 0.0240 M sodium acetate to raise thepH to 5.75?4th attempt>3rd attempt2nd attemptmL*510 QUESTIONS COMPLETEDVIEW SOLUTIONSUBMIT ANSWER

Answered: 06 Question (1 point) See page 768…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 10ALQ

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. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
8-55 We commonly refer to a buffer as consisting of approximately equal molar amounts of a weak acid and its conjugate base—for example, CH3COOH and CH3COO-. Is it also possible to have a buffer consisting of approximately equal molar amounts of a weak base and its conjugate acid? Explain.
Calculate the pH after 0.010 mole of gaseous HCl is added to 250.0 mL of each of the following buffered solutions. a. 0.050 M NH3/0.15 M NH4Cl b. 0.50 M NH3/1.50 M NH4Cl Do the two original buffered solutions differ in their pH or their capacity? What advantage is there in having a buffer with a greater capacity?
Calculate the pH after 0.15 mole of solid NaOH is added to 1.00 L of each of the following solutions: a. 0.050 M propanoic acid (HC3H5O2, Ka = 1.3 105) and 0.080 M sodium propanoate b. 0.50 M propanoic acid and 0.80 M sodium propanoate c. Is the solution in part a still a buffer solution after the NaOH has been added? Explain.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
Calculate the pH of a buffer solution prepared from 0.155 mol of phosphoric acid, 0.250 mole of KH2PO4, and enough water to make 0.500 L of solution.
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
A 80.0 mL sample of 0.0200 M HCI is titrated with 0.0400 M KOH solution. Calculate the pH after the following volumes of base have been added. 6 19 (a) 17.2 mL (b) 39.2 mL (c) 40.0 mL pH= pH= pH = (d) 42.0 mL (e) 68.8 mL pH = pH = Hom Rece My s ook Ch 2: Us eacti Fe (2
Write the reaction that occurs and calculate the pH after... 15.0 mL of 0.100 M NaOH is added to 5.00 mL of 0.150 M HCl 25.0mLof0.10MNaOHisaddedto40.0mLof0.20MHF. (Ka 3.5x10-4) 80.0mLof0.10MNaOHisaddedto40.0mLof0.20MHF. (Ka 3.5x10-4)
A buffer solution could be made by mixing equal amounts of citric acid and a solution containing. would resist When a small amount of strong acid or base is added, this buffer The statements above are completed by ཤ (-) (-C,H,O(C00), tay ila pH change (aq) i-C,H,O(COO), (aq) О -C,H,O(COOH),COO) О i-C,H,O(COOH),C00(a) it an equilibrium shift -a pH change -an equilibrium shift
www.riverbe * Question Completion Status: East Alton M QUESTION 6 Select any systems that could be used to buffer a solution at a pH of 6. Mark all appropriate answers. O NH4NH3 Ka-5.6 x 10-10 O HCO37CO32 K=4.8 x 10-11 O CgHsCOOH/CgHgCOO Ka=6.46 x 10-5 O HSO47SO,2- Ka=1.02 x 10-7 O H2CO3/HCO3 K4.3 x 107 O HFIF K= 7.2 x 104 QUESTION 7 What would the base/acid ratio be for the CH3COOH I CH3C00" system in order to create a pH 5.7? Round to two decimal places. QUESTION 8 6. How many grams of NH4CI must be added to 0.100 L of 0.445 M NH3 to produce a buffer solution with pH= 9.37 ? pKa (NH¼CI) = 9.24 Units are not required on the answer. Round your answer to two decimal places.

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