(a) Please write the conjugate bases of the following acids. (1) CH3COOH - CH3CO0 (Ka = 1.76 x 10-5) pka= 4.75 (2) HCIO2 → Clo2 (Ka = 1.09 x 10-2) pka = 1.96 (3) NHA - NHs (Ka = 5.66 x 10-10) pka = 9.as (4) HCIO - CIo (Ka = 2.91 x 10-8) pka = 7, 54 (b) If you are asked to design a buffer solution of pH = 2.30. Which one of the four above systems would you choose to have the best performance as the buffer? Cbasel PH = pka + log [acid] (a) = 230 = 1.96 + log TAS O 2.30 = 4.75+log CAJ 2.18 = CA) HCIO2 & CIO2 [8] CB] -a.45 = log CA) (3) = a.30 = 4.as+ log CAJ CB3 1.12 x 10-7= CAJ 0.003S = CA3 CB) (4) = a.30 = 7.54 + log CAJ 5.75K106= CA) (c) Calculate the molar ratio of buffer components for the system you choose. [B] CA] LIO. HCIO2 : a.18 (A] HUO, %3D 46 %3D [B] C10, 2.18 (d) If you want the pH value change to be less than 0.10 for a 2.00 L buffer solution after adding 0.20 moles of a strong base, e.g. NaOH (suppose no total volume change for the buffer solution), what would be the minimum amount of acid in moles needed to make the buffer solution?
(a) Please write the conjugate bases of the following acids. (1) CH3COOH - CH3CO0 (Ka = 1.76 x 10-5) pka= 4.75 (2) HCIO2 → Clo2 (Ka = 1.09 x 10-2) pka = 1.96 (3) NHA - NHs (Ka = 5.66 x 10-10) pka = 9.as (4) HCIO - CIo (Ka = 2.91 x 10-8) pka = 7, 54 (b) If you are asked to design a buffer solution of pH = 2.30. Which one of the four above systems would you choose to have the best performance as the buffer? Cbasel PH = pka + log [acid] (a) = 230 = 1.96 + log TAS O 2.30 = 4.75+log CAJ 2.18 = CA) HCIO2 & CIO2 [8] CB] -a.45 = log CA) (3) = a.30 = 4.as+ log CAJ CB3 1.12 x 10-7= CAJ 0.003S = CA3 CB) (4) = a.30 = 7.54 + log CAJ 5.75K106= CA) (c) Calculate the molar ratio of buffer components for the system you choose. [B] CA] LIO. HCIO2 : a.18 (A] HUO, %3D 46 %3D [B] C10, 2.18 (d) If you want the pH value change to be less than 0.10 for a 2.00 L buffer solution after adding 0.20 moles of a strong base, e.g. NaOH (suppose no total volume change for the buffer solution), what would be the minimum amount of acid in moles needed to make the buffer solution?
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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a - c are correct. Please help with part d.
![(a) Please write the conjugate bases of the following acids.
(1) CH3COOH →
CH3CO0
(Ka = 1.76 x 105) pKa = 4.75
(2) HCIO2
Clo2
(Ka = 1.09 x 10-2) pka = 1.96
(3) NHa+
NH3
(Ka = 5.66 x 10-10) pka = 9.as
(4) HCIO
CIo-
(Ka = 2.91 x 108) pka = 7, 54
(b) If you are asked to design a buffer solution of pH = 2.30. Which one of the four above systems
would you choose to have the best performance as the buffer?
(8)
(a) = 2.30 = 1.96 + log TA
Cbasel
PH = pka + log Tacid]
CB)
CA)
३.18 =
[B]
O 2.30 = 4.75 + log
HCIO2 & CIO2
CAJ
(3) = a.30 = 9.2s+ log CAJ
- a.45 = log CAJ
CB3
CAJ
CB]
(4) = a.30 = 7.S4 + log
CAJ
1.12 x 10-72
0.003S =
CA3
5.75K10-6=
CA)
(c) Calculate the molar ratio of buffer components for the system you choose.
[B]
CAJ
LIO
- a.18
HCIO
CA]
46
[B]
2.18
(d) If you want the pH value change to be less than 0.10 for a 2.00 L buffer solution after adding 0.20
moles of a strong base, e.g. NaOH (suppose no total volume change for the buffer solution), what
would be the minimum amount of acid in moles needed to make the buffer solution?
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Transcribed Image Text:(a) Please write the conjugate bases of the following acids.
(1) CH3COOH →
CH3CO0
(Ka = 1.76 x 105) pKa = 4.75
(2) HCIO2
Clo2
(Ka = 1.09 x 10-2) pka = 1.96
(3) NHa+
NH3
(Ka = 5.66 x 10-10) pka = 9.as
(4) HCIO
CIo-
(Ka = 2.91 x 108) pka = 7, 54
(b) If you are asked to design a buffer solution of pH = 2.30. Which one of the four above systems
would you choose to have the best performance as the buffer?
(8)
(a) = 2.30 = 1.96 + log TA
Cbasel
PH = pka + log Tacid]
CB)
CA)
३.18 =
[B]
O 2.30 = 4.75 + log
HCIO2 & CIO2
CAJ
(3) = a.30 = 9.2s+ log CAJ
- a.45 = log CAJ
CB3
CAJ
CB]
(4) = a.30 = 7.S4 + log
CAJ
1.12 x 10-72
0.003S =
CA3
5.75K10-6=
CA)
(c) Calculate the molar ratio of buffer components for the system you choose.
[B]
CAJ
LIO
- a.18
HCIO
CA]
46
[B]
2.18
(d) If you want the pH value change to be less than 0.10 for a 2.00 L buffer solution after adding 0.20
moles of a strong base, e.g. NaOH (suppose no total volume change for the buffer solution), what
would be the minimum amount of acid in moles needed to make the buffer solution?
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