Why can a buffer be prepared from a mixture of NH4Cl and NaOH but not from NH3and NaOH? Question 26 options: a) OH– is a weak base, and NH4+ is a strong base. They react with one another to form NH3, thereby setting up the equilibrium NH4+(aq) + OH-(aq) ⇌ NH3(aq) + H2O(l). Because both are acids, a buffer is formed. However, in the second case, NH3 is a base and OH– is an acid, so no buffer is possible. b) OH– is a weak base, and NH4+ is a strong base. They react with one another to form NH3, thereby setting up the equilibrium NH4+(aq) + OH-(aq) ⇌ NH3(aq) + H2O(l). Because both are bases, a buffer is formed. However, in the second case, NH3 is an acid and OH– is a base, so no buffer is possible. c) OH– is a base, and NH4+ is a strong acid. They react with one another to form NH3, thereby setting up the equilibrium NH4+(aq) + OH-(aq) ⇌ NH3(aq) + H2O(l). Because both the base (NH3) and the conjugate acid (NH4+) are present, a buffer is formed. However, in the second case, NH3 and OH– are both acids, so no buffer is possible. d) OH– is a base, and NH4+ is a weak acid. They react with one another to form NH3, thereby setting up the equilibrium NH4+(aq) + OH-(aq) ⇌ NH3(aq) + H2O(l). Because both the base (NH3) and the conjugate acid (NH4+) are present, a buffer is formed. However, in the second case, NH3 and OH– are both bases, so no buffer is possible.

Buffer Solution is a water solvent based solution which consists of a mixture containing a weak acid…

Answered: up the equilibrium NH4+(aq) + OH-(aq) ⇌…

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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Why can a buffer be prepared from a mixture of NH₄Cl and NaOH but not from NH₃and NaOH?

Question 26 options:

OH^– is a weak base, and NH₄⁺ is a strong base. They react with one another to form NH₃, thereby setting up the equilibrium NH₄⁺_(aq) + OH^-(aq) ⇌ NH_3(aq) + H₂O_(l). Because both are acids, a buffer is formed. However, in the second case, NH₃ is a base and OH^– is an acid, so no buffer is possible.

OH^– is a weak base, and NH₄⁺ is a strong base. They react with one another to form NH₃, thereby setting up the equilibrium NH₄⁺_(aq) + OH^-(aq) ⇌ NH_3(aq) + H₂O_(l). Because both are bases, a buffer is formed. However, in the second case, NH₃ is an acid and OH^– is a base, so no buffer is possible.

OH^– is a base, and NH₄⁺ is a strong acid. They react with one another to form NH₃, thereby setting up the equilibrium NH₄⁺_(aq) + OH^-(aq) ⇌ NH_3(aq) + H₂O_(l). Because both the base (NH₃) and the conjugate acid (NH₄⁺) are present, a buffer is formed. However, in the second case, NH₃ and OH^– are both acids, so no buffer is possible.

OH^– is a base, and NH₄⁺ is a weak acid. They react with one another to form NH₃, thereby setting up the equilibrium NH₄⁺_(aq) + OH^-(aq) ⇌ NH_3(aq) + H₂O_(l). Because both the base (NH₃) and the conjugate acid (NH₄⁺) are present, a buffer is formed. However, in the second case, NH₃ and OH^– are both bases, so no buffer is possible.

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