Use the References to access important values if needed for this question.Design a buffer that has a pH of 5.86 using one of the weak base/conjugate acid systems shown below.Weak BaseCH3NH2C6H1503NC5H5NKb4.2x10-4 CH3NH3+5.9x10-7 C6H1503NH+1.5×10-9 C5H5NH*Submit AnswerConjugate AcidHow 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 acidgrams weak base =Kapka2.4x10-11 10.621.7x10-8 7.776.7x10-6 5.17=Retry Entire Group 2 more group attempts remaining

Given,The pH of the buffer solution = 5.86Volume of buffer solution = 1.00 LConcentration of the…

Use the References to access important values if needed for this question. Design a buffer that has a pH of 5.86 using one of the weak base/conjugate acid systems shown below. Weak Base CH3NH₂ C6H1503N C5H5N Kb 4.2x10-4 CH3NH3+ 5.9x10-7 C6H1503NH+ 1.5x10-9 C5H5NH+ Conjugate Acid Submit Answer 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 = Ka pka 2.4x10-11 10.62 1.7x10-8 7.77 6.7x10-6 5.17 Retry Entire Group 2 more group attempts remaining

Use the References to access important values if needed for this question. Design a buffer that has a pH of 5.86 using one of the weak base/conjugate acid systems shown below. Weak Base CH3NH₂ C6H1503N C5H5N Kb 4.2x10-4 CH3NH3+ 5.9x10-7 C6H1503NH+ 1.5x10-9 C5H5NH+ Conjugate Acid Submit Answer 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 = Ka pka 2.4x10-11 10.62 1.7x10-8 7.77 6.7x10-6 5.17 Retry Entire Group 2 more group attempts remaining

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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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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show calculations for how the pH of each of these solutions would be determined. a. Buffer solution prepared from 10.00 mL of 1.0 M HC2H3O2 and 10.00 mL of 1.0 M NaC2H3O2 b. 20.00 mL of buffer solution with 1.00 mL of 1.0 M NaOH. c. 20.00 mL of buffer solution with 1.00 mL of 1.0 M HCl. d. 20.00 mL of water with 1.00 mL of 1.0 M NaOH added e. 20.00 mL of water with 1.00 mL of 1.0 M HCl added
III. Acids, Bases, Buffers: 1. Using following equation, explain how buffers work. НА - H+ Proton Conjugate Ba se Acid
please answer both for a vote uofront. thanks (Please type answer no write by hend)
Which of the following is not a characteristic of buffer solutions? O They cannot be tailored to maintain a specified pH. O They contain a conjugate base of a weak acid. O They contain a weak acid. O They have a finite capacity for accommodating added acid or base. O They can maintaln their pH, even when small amounts of acid or base are added. QUESTION 10 The capacity of a buffer solution is greater when there are large amounts of a weak acid and its conjugate base in solution. O True O False
Which of the following solutions can act as a buffer? HCI and NACI NaCl and H2O NaOH and HCI NH3 and NH,CI
Ethyl orange changes from red at 3.4 to blue at 4.8. What is the approximate Kin value for ethyl orange? 1.3E4 1.6E -5 4.1 4.0E-4 7.9 8E-5 What form is the indicator in if the pH is 6? In-, the deprotonated form Hln, the protonated form a mixture of both Hin and In -
Which of the following acid/base pairs would not make a good buffer system? H2PO4-/ HPO42- HSO3-/Na2SO3 H2CO3/H2CO2- NH4+/NH3 HNO2/NO2-
Determine the resulting pH when 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C6H5NH3CI and 0.500 M C6H5NH2. The value of Kb for C6H5NH2 is 4.3 x 101°. 1 2 3 4 NEXT Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. C6H;NH3*(aq) Он (aq) H20(1) C6H;NH2(aq) + + Before (mol) Change (mol) After (mol) 5 RESET 0.040 -0.040 0.500 -0.500 0.100 -0.100 +x 0.040 + x 0.040 - x 0.100 + x 0.100 - x 0.060 -0.060 -x 0.140 -0.140 0.020 -0.020
Solve correctly please , need both subparts to be solve.