Question

6. Which of the following acids and its conjugate base would be the best buffer to maintain a pH at 7.50? (1pt) Potassium hydrogen sulfite, KHSO$_3$, K$_a$ = 6.4x10$^{-8}$ Potassium hydrogen sulfate, KHSO$_4$, K$_a$ = 1.2x10$^{-2}$ Potassium hydrogen phthalate, KHC$_8$H$_4$O$_4$, K$_a$ = 3.0x10$^{-6}$ Potassium hydrogen tartrate, KHC$_4$H$_4$O$_6$, K$_a$ = 4.6x10$^{-5}$ Write the chemical formulas for the two components of this buffer: (2pts) Propose acceptable concentrations for each component of this buffer if it needs to have a buffering capacity of .0500 M of added strong acid/base. (1pt) Write the net ionic equation for the reaction of this buffer as it neutralizes added strong base.(1 pt) Write the net ionic equation for the reaction of this buffer as it neutralizes added strong acid. (1 pt)

          6. Which of the following acids and its conjugate base would be the best buffer to maintain a pH at 7.50? (1pt)
Potassium hydrogen sulfite, KHSO$_3$, K$_a$ = 6.4x10$^{-8}$ 
Potassium hydrogen sulfate, KHSO$_4$, K$_a$ = 1.2x10$^{-2}$
Potassium hydrogen phthalate, KHC$_8$H$_4$O$_4$, K$_a$ = 3.0x10$^{-6}$
Potassium hydrogen tartrate, KHC$_4$H$_4$O$_6$, K$_a$ = 4.6x10$^{-5}$ 
Write the chemical formulas for the two components of this buffer:
(2pts)
Propose acceptable concentrations for each component of this buffer if it needs to have a buffering capacity
of .0500 M of added strong acid/base. (1pt)
Write the net ionic equation for the reaction of this buffer as it neutralizes added strong base.(1 pt)
Write the net ionic equation for the reaction of this buffer as it neutralizes added strong acid. (1 pt)

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6. Which of the following acids and its conjugate base would be the best buffer to maintain a pH at 7.50? (1pt)
Potassium hydrogen sulfite, KHSO3, Ka = 6.4x10^-8
Potassium hydrogen sulfate, KHSO4, Ka = 1.2x10^-2
Potassium hydrogen phthalate, KHC8H4O4, Ka = 3.0x10^-6
Potassium hydrogen tartrate, KHC4H4O6, Ka = 4.6x10^-5
Write the chemical formulas for the two components of this buffer:
(2pts)
Propose acceptable concentrations for each component of this buffer if it needs to have a buffering capacity
of .0500 M of added strong acid/base. (1pt)
Write the net ionic equation for the reaction of this buffer as it neutralizes added strong base.(1 pt)
Write the net ionic equation for the reaction of this buffer as it neutralizes added strong acid. (1 pt)

Added by Vernon C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

07/09/2022

Step 1

50. - KHSO3: pKa = -log(6.4×10^-8) = 7.19 - KHSO4: pKa = -log(1.2×10^-2) = 1.92 - KHC8H4O4 (potassium hydrogen phthalate): pKa = -log(3.0×10^-6) = 5.52 - KHC4H4O6 (potassium hydrogen tartrate): pKa = -log(4.6×10^-5) = 4.34 The pKa closest to 7.50 is 7.19 (KHSO3), Show more…

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Please solve all parts of question 6: (a) Which of the following acids and its conjugate base would be the best buffer to maintain a pH at 7.50? Potassium hydrogen sulfite, KHSO3, Ka=6.4×10^(-8) Potassium hydrogen sulfate, KHSO4, Ka=1.2×10^(-2) Potassium hydrogen phthalate, KHC8H4O4, Ka=3.0×10^(-6) Potassium hydrogen tartrate, KHC4H1O6, Ka=4.6×10^(-5) (b) Write the chemical formulas for the two components of this buffer. (c) Propose acceptable concentrations for each component of this buffer if it needs to have a buffering capacity of 0.0500M of added strong acid/base. (d) Write the net ionic equation for the reaction of this buffer as it neutralizes added strong base. (e) Write the net ionic equation for the reaction of this buffer as it neutralizes added strong acid. 6. Which of the following acids and its conjugate base would be the best buffer to maintain a pH at 7.50? 1pt) Potassium hydrogen sulfite, KHSO3, Ka=6.4x10^(-8) Potassium hydrogen sulfate, KHSO4, Ka=1.2x10^2 Potassium hydrogen phthalate, KHC8H4O4, Ka=3.0x10 Potassium hydrogen tartrate, KHC4H1O6, Ka=4.6x10^5 (2pts) Write the chemical formulas for the two components of this buffer: of 0.0500M of added strong acid/base. (1pt)

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