© Macmillan Learning You need to prepare an acetate buffer of pH 5.36 from a 0.662 M acetic acid solution and a 2.13 M KOH solution. If you have 580 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 5.36? The pK, of acetic acid is 4.76. Be sure to use appropriate significant figures. 710 Incorrect mL

© Macmillan Learning You need to prepare an acetate buffer of pH 5.36 from a 0.662 M acetic acid solution and a 2.13 M KOH solution. If you have 580 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 5.36? The pK, of acetic acid is 4.76. Be sure to use appropriate significant figures. 710 Incorrect mL

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

Part A B and C
One Erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other Erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HCl (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used? please explain than solve
Tu Please don't provide the handwriting solution
Please answer both parts.
The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.500 moles of a monoprotic weak acid (?a=8.9×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point? pH= ( Please type answer note write by hend )
Give typed full explanation not a single word hand written otherwise leave it
determine the volume of 0.2 M sodium acetate required to be added to prepapre 100 mL of 0.2 M acetate buffer at ph 4.2? Use the table as a reference.
If a 0.552M HCl caq) solution is used by a scientist to titrate 10.00mL of a weak base, based curve (shown below), what base? write your the titration the concentration of the auswer with 4 decitual places. pH Curve OM is 12 10 8 6 4 2 0 5:0 2 1.5 n 3 3.5 A Volume of Titrant / mL 7.5 8 8.5
please don't provide handwritten solution..
Paylben
ortant values if needed for this question. Design a buffer that has a pH of 4.66 using one of the weak base/conjugate acid systems shown below. Ka pka 2.4x10-11 10.62 1.7x10-8 7.77 6.7x10-6 5.17 Weak Base Kb Conjugate Acid 4.2x 10-4 CH3NH3+ CH3NH₂ C6H1503N 5.9x107 C6H1503NH+ C5H5N 1.5x109 C5H5NH+ How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams chloride salt of conjugate acid = grams weak base =
You need to prepare an acetate buffer of pH 5.18 from a 0.735 M acetic acid solution and a 2.05 M KOH solution. If you have 630 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 5.18? The pK, of acetic acid is 4.76. Be sure to use appropriate significant figures. 5.94 mL Incorrect insert prt scr delete $ 7 8 [9 + backspace 5 8 home %3D [4 (5) R T Y 1O P pg u [ 2 K 3 F G J enter pause B M ↑ shift alt ctrl