Chem 129 Topic Set 7 Variations of titration and Buffers G. How would you make 350mL of a buffer with a total concentration of 0.75M and a pH of 9.00 from the list of materials below? (your answer should include the volumes of two solutions and the amount of DI water needed to reach the total volume) [remember: vol* total conc->total moles->moles weak, targetpH->ratio->stoich->moles strong] i. A solution of 1.25 M hydrochloric acid ii. A solution of 1.25 M sodium hydroxide iii. A solution of 1.25 M chloroacetic acid (pKa = 2.85) iv. A solution of 1.25 M ammonia (pka = 9.25) v. A solution of 1.25 M carbonic acid (pKa1 = 6.37, pKa2 = 10.32 vi. A solution of 1.25 M acetic acid (pka = 4.75) Ditutionen 1) What would be the volume of weak component and what would be the volume of strong component? MV MV (0.75) (350) = 1.25 (x) ne modified x = 210 mL 2) What would be the capacity of the buffer? 3) After the buffer is made, what would the pH change to if 24.5mL of 1.25 M hydrochloric acid is added? 4) After the buffer is made, what would PH to IF 37.3 mL of 1.25 M sodium was added change hydroxide

Chem 129 Topic Set 7 Variations of titration and Buffers G. How would you make 350mL of a buffer with a total concentration of 0.75M and a pH of 9.00 from the list of materials below? (your answer should include the volumes of two solutions and the amount of DI water needed to reach the total volume) [remember: vol* total conc->total moles->moles weak, targetpH->ratio->stoich->moles strong] i. A solution of 1.25 M hydrochloric acid ii. A solution of 1.25 M sodium hydroxide iii. A solution of 1.25 M chloroacetic acid (pKa = 2.85) iv. A solution of 1.25 M ammonia (pka = 9.25) v. A solution of 1.25 M carbonic acid (pKa1 = 6.37, pKa2 = 10.32 vi. A solution of 1.25 M acetic acid (pka = 4.75) Ditutionen 1) What would be the volume of weak component and what would be the volume of strong component? MV MV (0.75) (350) = 1.25 (x) ne modified x = 210 mL 2) What would be the capacity of the buffer? 3) After the buffer is made, what would the pH change to if 24.5mL of 1.25 M hydrochloric acid is added? 4) After the buffer is made, what would PH to IF 37.3 mL of 1.25 M sodium was added change hydroxide

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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he X - OWLV2 | Assigr x : OWLV2 | Online X y! google - Yahoc X e Registration - L X O selfserve.una.e X Irn/takeAssignment/takeCovalentActivity.do?locator=assignment-take [Review Topics] [References) Use the References to access important values if needed for this question. A buffer solution is 0.478 M in H2SO3 and 0.380 M in KHSO3. If K for H2SO3 is 1.7 x 10-2, what is the pH of this buffer solution? pH = Submit Answer Retry Entire Group 9 more group attempts remaining 5:05 P 11/2/20 Cop fi2 ort sc delete home ho backspace num Iock
Chapter 17 Multiple Choice Question 21 13 of 16 <. I Review | Constants | Periodic Table Part A A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 x 10-4. O 2.89 О 334 О 357 О 3.63 О 346
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HOWICX S Geometry w/Datax S Practice 10.10 | Sex S Practice | SchoolcX G Sign in - Google/X Logins & Passwo X + gagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator= assignment-take ★ Other Booki [Review Topics] [References] Use the References to access important values if needed for this question. A buffer solution contains 0.493 M C6H5NH3Br and 0.337 M C6H5NH2 (aniline). Determine the pH change when 0.088 mol NaOH is added to 1.00 L of the buffer. pH after addition - pH before addition = pH change Submit Answer Retry Entire Group 1 more group attempt remaining HANA D ?? ak
Consider titration of 25 mL of .IM CH₂ CO₂H with 1 M NaOH. Calculate the pH after the following volumes of NaOH: adding a) O mL b) 12.5 mL c) 25mL d) 37.5 mL
ts eBook Print ferences This question has three parts. Be sure to answer all parts. Calculate and compare the molar solubility of Mg(OH)₂ in water and in a solution buffered at a pH of 5.5. Part 1 out of 3 (a) Determine the molar solubility of Mg(OH)₂ in water and the pH of a saturated Mg(OH)₂ solution. molar solubility 1.6 pH=10.51 2 attempts left B Check my work Next part Hint Solutia Guided So
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If we would like to make a 1 L buffer solution with 0.1 M concentration with a pH value of 7.0 usingand KH2PO4 and K3PO4, how many grams of each reagent do we need?
23. In a titration, 30mL of 1.5 M KOH are added to 15.0 ml of 3.0 M HNO3. This titration has _____ the equivilance point and the pH in resulting solution is. a. gone beyond, greater than 7 b. reaced, greater than 7 c. not yet reached, less than 7 d. reached, 7