A group of students were able to isolate a novel amylase from the saliva of a pig found inCountry Aeros. In the process of isolating the novel saliva amylase, the students wanted toprepare 250 mL of 1.0 M phosphate buffer with a pH = 7.4. (AW (g/mol): Na = 23.10, H = 1.01,P = 30.97, O=16.00)Base from this table, what buffer system - acid, conjugate base- is most suitable to prepare thebuffer?AcidКаH3PO41x10з6.3 х108HPO,?4.2 x 10-13

Given the desired pH = 7.4 We can find the most suitable buffer based on the Henderson equation.

Answered: A group of students were able to…

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...

See similar textbooks

Similar questions

A chemistry graduate student is given 500. mL of a 1.50M trimethylamine ((CH3)N solution. Trimethylamine is a weak 4 base with K, =7.4 × 10 *. what mass of (CH, NHB should the student dissolve in the (CH,) N solution to turn it into a 3 buffer with pH = 10.62? %3D You may assume that the volume of the solution doesn't change when the (CH,) NHB is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
please do only the highlighted qouestion
An undergraduate research student wishes to create a system that mimics human blood (pH = 7.4). The student chose as the model system to use a buffer solution of sodium dihydrogen phosphate (NaH2PO4, Ka = 6.2 × 10–8) and sodium hydrogen phosphate (Na2HPO4, Ka = 4.2 × 10-13). A) Which of the components of the buffer solution is the acid? B) Using the Henderson Hasselbalch equation, calculate the mole ratio of Na2HPO4/NaH2PO4 the student needs to use. C) To approximate the human condition of blood alkalosis (where the pH of blood rises to 7.6, which is usually lethal), how much base will the student need to add to the buffer?
-5 %3D A chemistry graduate student is given 450. mL of a 0.30 M acetic acid (HCH,CO,) solution. Acetic acid is a weak acid with K = 1.8 × 10 . What mass of a NaCH,CO, should the student dissolve in the HCH,CO, solution to turn it into a buffer with pH =4.29? 2
-3 A chemistry graduate student is given 450. mL of a 1.10M diethylamine ((C₂H), NH) solution. Diethylamine is a weak base with K₂ = 1.3 × 10¯ What mass of (C₂H₂)2NH₂Cl should the student dissolve in the (C₂H5) NH solution to turn it into a buffer with pH = 11.25? You may assume that the volume of the solution doesn't change when the (C₂H5) NH₂Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 Explanation 85°F Mostly sunny Check $ D x10 X C % S E F6 Q Search. F7 & L FB a * F9 F10 Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessi *- F11 *+ F12 PrtSc Insert Delete 4)
33.) A buffer solution contains 0.45 mol of hydrazoic acid (HN3) and 0.28 mol of sodium hydrazoate (NaN3) in 8.60 L. The Ka of hydrazoic acid (HN3) is Ka = 1.9e- 05. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.15 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the addition of 0.25 mol of HI? (assume no volume change)
7) How many mL of 1.778 M HCl should be added to 355 mL of 0.282 M aminobenzene (ABz), a weak base, before diluting to 1 L to prepare a buffer at pH 4.44? pKa= 4.601 HABz+ NA
Consider the titration of 15.75 mL of 0.549 M potassium propanoate, CH3CH,CO,K, with 0.207 M HNO3. What is the pH of the solution after 39.83 mL of the HNO3 has been added? (pK, of CH;CH-COH = 4.691)
5
2. Joey was tasked to ensure that an enzyme responsible for keeping his species from extinction remains biologically active. To do so, he needs to store it in a buffer solution with a pH of 10.00. Unfortunately, only three buffer systems are available in their laboratory: Buffer System Weak Acid Component Ka Conjugate Base Salt KYA Benzoic acid, C6H5COOH 6.25 x 105 NaCH₂COO MUH Boric acid, H3BO3 5.81 x 107 NaH₂BO TWO Hydrogen cyanide, HCN 6.20 X 10-10 NaCN A. In what buffer system (KYA, MUH, or TWO) will Joey store the enzyme? In your solution sheet, show calculations and briefly explain to support your answer. B. Write the equilibrium reaction involved in the buffer system. Write your answer on your solution sheet C. Calculate the amount (in mL) of the 1.75 M stock solution (pH 7.00) of the same buffer system needed to prepare 250 mL of a 0.550 M buffer pH 7.00. After preparing the buffer, Joey decided to determine the buffer capacity of the solution by titration using 0.500 M NaOH as…
(5e) Which two of the following compounds would you make a buffer of pH = 12.5. H3PO4 (MM=98.00 g/mol), NaH2PO4 (MM=119.98 g/mol), NazHPO4 (MM=141.96 g/mol), and Na3PO4 (MM = 163.94 g/mol)? [For H3PO4: pK; = 2.148; pKz=7.199; pK3=12.15]
You are tasked with making a buffer solution containing equal amounts of propionic acid from a 99.5 wt% solution (d = 0.993 g/mL, FW = 74.08 g/mol) and sodium propionate (solid, FW = 96.06 g/mol). What concentration of the buffer must be prepared to prevent a change in the pH by more than 0.5 pH units after the addition of 10.00 mL of 3.00 M HCl to 100.0 mL of the buffer solution? The Ka for propionic acid is 1.76 x 10-5.

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS