Which is the best solution to buffer at pH = 10.50? (A) A buffer solution containing 0.25 M H2CO3 and 0.45 M Na2CO3; (Ka (H2CO3) = 4.3 x 10–7) (B) A buffer solution containing 0.25 M NaHCO3 and 0.45 M Na2CO3; (Ka (HCO3–) = 5.6 x 10–11) (C) A buffer solution containing 0.12 M NaHCO3 and 0.22 M Na2CO3; (Ka (HCO3–) = 5.6 x 10–11) (D) A buffer solution containing 0.12 M NH4Cl and 2.2 M NH3; (Ka (NH4+) = 5.6 x 10–10)

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Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter8: Acids And Bases

Section: Chapter Questions

Problem 8.104P

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Question

Which is the best solution to buffer at pH = 10.50?

(A) A buffer solution containing 0.25 M H₂CO₃ and 0.45 M Na₂CO₃; (K_a (H₂CO₃) = 4.3 x 10^–7)

(B) A buffer solution containing 0.25 M NaHCO₃ and 0.45 M Na₂CO₃; (K_a (HCO₃^–) = 5.6 x 10^–11)

(D) A buffer solution containing 0.12 M NH₄Cl and 2.2 M NH₃; (K_a (NH₄⁺) = 5.6 x 10^–10)

Expert Solution

Step 1

Henderson-Hasselbalch equation

The equation that is used to calculate the pH of a buffer solution is called Henderson-Hasselbalch equation.

The equation is ;

For an acidic buffer,

$\begin{array}{rcl} pH & = & {pK}_{a} + \log \frac{[conjugate base]}{[acid]} \\ [conjugate base] & = & concentration of conjugate base \\ [acid] & = & concentration of acid \end{array}$

For a basic buffer,

$\begin{array}{rcl} pOH & = & {pK}_{b} + \log \frac{[conjugate acid]}{[base]} \\ [conjugate acid] & = & concentration of conjugate acid \\ [base] & = & concentration of base \end{array}$

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