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A buffer is made by mixing 5.0 mL of 3.0 M NH,(aq) with 10 mL of 1.44 M NH C(aq). What is the pH of the buffer at 25°C, if the base ionization constant of ammonia is 1.8×10- and the ion product of water is 1.0x10-14 at this temperature?. Enter your answer in the box provided with correct units and sig. figs.: Comment : Henderson-Hasselbalch equations for acidic and basic buffers are listed on the next page. Answer: pH,uffer %3D

A buffer is made by mixing 5.0 mL of 3.0 M NH,(aq) with 10 mL of 1.44 M NH C(aq). What is the pH of the buffer at 25°C, if the base ionization constant of ammonia is 1.8×10- and the ion product of water is 1.0x10-14 at this temperature?. Enter your answer in the box provided with correct units and sig. figs.: Comment : Henderson-Hasselbalch equations for acidic and basic buffers are listed on the next page. Answer: pH,uffer %3D

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Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Page 272 Henderson-Hasselbalch Equations Equilibrium equation for acidic buffer containing weak acid, HB(aq), and its conjugate base, B (aq), and governed by acid ionization constant K, is written as: + HB(aq) + H,O() B (aq) + H,O*(aq), K = (1HB), - [*,0°]) If both initial concentrations, [HB], and [B-1,> K, and at the same time K, << 1, then the pH of the buffer solution is calculated as: pH, %3D "buffer pK, + log [HB], Equilibrium equation for basic buffer containing weak base, B(aq), and its conjugate acid, BH" (aq), and governed by base ionization constant K, is written as: ([a* ]o • [Ox"])[on"] (18), - [OH"]) B(aq) + H,O) 2 BH"(aq) + OH (aq), %3D If both initial concentrations, [B], and BH* Jo >> K,, and at the same time K, << 1, then the pH of the buffer solution is calculated as: BH 0 'buffer pKw- pK,- log [B], pH, %3D
Transcribed Image Text:Page 272 Henderson-Hasselbalch Equations Equilibrium equation for acidic buffer containing weak acid, HB(aq), and its conjugate base, B (aq), and governed by acid ionization constant K, is written as: + HB(aq) + H,O() B (aq) + H,O*(aq), K = (1HB), - [*,0°]) If both initial concentrations, [HB], and [B-1,> K, and at the same time K, << 1, then the pH of the buffer solution is calculated as: pH, %3D "buffer pK, + log [HB], Equilibrium equation for basic buffer containing weak base, B(aq), and its conjugate acid, BH" (aq), and governed by base ionization constant K, is written as: ([a* ]o • [Ox"])[on"] (18), - [OH"]) B(aq) + H,O) 2 BH"(aq) + OH (aq), %3D If both initial concentrations, [B], and BH* Jo >> K,, and at the same time K, << 1, then the pH of the buffer solution is calculated as: BH 0 'buffer pKw- pK,- log [B], pH, %3D
A buffer is made by mixing 5.0 mL of 3.0 M NH,(aq) with 10 mL of 1.44 M NH Cl(aq). What is the pH of the buffer at 25°C, if the base ionization constant of ammonia is 1.8x10° and the ion product of water is 1.0x10-14 at this temperature?. Enter your answer in the box provided with correct units and sig. figs.: Comment : Henderson-Hasselbalch equations for acidic and basic buffers are listed on the next page. Answer: pH, 'buffer
Transcribed Image Text:A buffer is made by mixing 5.0 mL of 3.0 M NH,(aq) with 10 mL of 1.44 M NH Cl(aq). What is the pH of the buffer at 25°C, if the base ionization constant of ammonia is 1.8x10° and the ion product of water is 1.0x10-14 at this temperature?. Enter your answer in the box provided with correct units and sig. figs.: Comment : Henderson-Hasselbalch equations for acidic and basic buffers are listed on the next page. Answer: pH, 'buffer
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