A chemistry graduate student is given 500. mL of a 0.40M ammonia (NH,) solution. Ammonia is a weak base with K,=1.8 × 10 What mass of NH,Cl should the student dissolve in the NH, solution to turn it into a buffer with pH =8.99? You may assume that the volume of the solution doesn't change when the NH,Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.

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...
icon
Related questions
Question
**Buffer Solution Calculation**

**Problem Statement:**
A chemistry graduate student is given 500. mL of a 0.40 M ammonia (NH₃) solution. Ammonia is a weak base with \( K_b = 1.8 \times 10^{-5} \). What mass of NH₄Cl should the student dissolve in the NH₃ solution to turn it into a buffer with \( \text{pH} = 8.99 \)?

**Assumptions:**
- The volume of the solution does not change when NH₄Cl is dissolved.
- Provide the answer in units and rounded to 2 significant digits.

In the given image, there appears to be a placeholder input field and multiple choice interaction widgets below the problem statement, which typically might be used in an online learning platform to capture students' calculations or responses.

To solve this problem, we can follow these steps:

1. **Write the Chemical Equilibrium Expression for NH₃:**
   \[ \text{NH₃} + \text{H₂O} \rightleftharpoons \text{NH₄}^+ + \text{OH}^- \]

2. **Calculate the pOH and [OH⁻]:**
   \[ \text{pH} = 8.99 \]
   \[ \text{pOH} = 14 - \text{pH} \]
   \[ \text{pOH} = 14 - 8.99 = 5.01 \]
   \[ [\text{OH}^-] = 10^{-\text{pOH}} = 10^{-5.01} \]

3. **Calculate the [NH₄⁺]:**
   Using the Henderson-Hasselbalch equation for bases:
   \[ \text{pOH} = \text{p}K_b + \log\left(\frac{[\text{NH₄}^+]}{[\text{NH₃}]}\right) \]
   Rearrange to find \([\text{NH₄}^+]\):
   \[ 5.01 = -\log(1.8 \times 10^{-5}) + \log\left(\frac{[\text{NH₄}^+]}{0.40}\right) \]
   Calculate \(\text{p}K
Transcribed Image Text:**Buffer Solution Calculation** **Problem Statement:** A chemistry graduate student is given 500. mL of a 0.40 M ammonia (NH₃) solution. Ammonia is a weak base with \( K_b = 1.8 \times 10^{-5} \). What mass of NH₄Cl should the student dissolve in the NH₃ solution to turn it into a buffer with \( \text{pH} = 8.99 \)? **Assumptions:** - The volume of the solution does not change when NH₄Cl is dissolved. - Provide the answer in units and rounded to 2 significant digits. In the given image, there appears to be a placeholder input field and multiple choice interaction widgets below the problem statement, which typically might be used in an online learning platform to capture students' calculations or responses. To solve this problem, we can follow these steps: 1. **Write the Chemical Equilibrium Expression for NH₃:** \[ \text{NH₃} + \text{H₂O} \rightleftharpoons \text{NH₄}^+ + \text{OH}^- \] 2. **Calculate the pOH and [OH⁻]:** \[ \text{pH} = 8.99 \] \[ \text{pOH} = 14 - \text{pH} \] \[ \text{pOH} = 14 - 8.99 = 5.01 \] \[ [\text{OH}^-] = 10^{-\text{pOH}} = 10^{-5.01} \] 3. **Calculate the [NH₄⁺]:** Using the Henderson-Hasselbalch equation for bases: \[ \text{pOH} = \text{p}K_b + \log\left(\frac{[\text{NH₄}^+]}{[\text{NH₃}]}\right) \] Rearrange to find \([\text{NH₄}^+]\): \[ 5.01 = -\log(1.8 \times 10^{-5}) + \log\left(\frac{[\text{NH₄}^+]}{0.40}\right) \] Calculate \(\text{p}K
Expert Solution
steps

Step by step

Solved in 2 steps

Blurred answer
Knowledge Booster
Precipitation Titrations
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY