How many grams of NH4Br must be dissolved in 1.00L of water to produce a solution with pH = 5.16? The Kb of NH3 is equal to 1.8 x 10-5. 1 2 NEXT > Let x represent the original concentration of NH4* in the water. Based on the given values, set up the ICE table in order to determine the unknown. NH,*(aq) H20(1) H3O*(aq) NH3(aq) + Initial (M) |Change (M) Equilibriu m (M) RESET 1.00 5.16 1.8 x 10-5 2x 0.5x - -2x -0.5x 6.9 x 10-6 -6.9 x 10-6 0.709 -0.709 x + 6.9 x 10"6 -X x - 6.9 × 10-6 x + 0.709 x - 0.709
How many grams of NH4Br must be dissolved in 1.00L of water to produce a solution with pH = 5.16? The Kb of NH3 is equal to 1.8 x 10-5. 1 2 NEXT > Let x represent the original concentration of NH4* in the water. Based on the given values, set up the ICE table in order to determine the unknown. NH,*(aq) H20(1) H3O*(aq) NH3(aq) + Initial (M) |Change (M) Equilibriu m (M) RESET 1.00 5.16 1.8 x 10-5 2x 0.5x - -2x -0.5x 6.9 x 10-6 -6.9 x 10-6 0.709 -0.709 x + 6.9 x 10"6 -X x - 6.9 × 10-6 x + 0.709 x - 0.709
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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Question
![**Interactive Activity: Calculating the Grams of NH₄Br Needed**
**Problem Statement:**
How many grams of NH₄Br must be dissolved in 1.00 L of water to produce a solution with pH = 5.16? The Kb of NH₃ is equal to 1.8 × 10⁻⁵.
**Instructions:**
1. Use the ICE (Initial, Change, Equilibrium) table to determine the unknown concentration of NH₄⁺ in the solution.
2. Let x represent the initial concentration of NH₄⁺.
**Reaction:**
\[ \text{NH}_4^+(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{H}_3\text{O}^+(aq) + \text{NH}_3(aq) \]
**ICE Table Structure:**
| | NH₄⁺(aq) | + | H₂O(l) | ⇌ | H₃O⁺(aq) | + | NH₃(aq) |
|-------------------|------------|----|--------|----|----------|----|--------|
| Initial (M) | | | | | | | |
| Change (M) | | | | | | | |
| Equilibrium (M) | | | | | | | |
**Available Answer Options:**
- Variables:
- x
- 2x
- 0.5x
- Changes:
- -x
- -2x
- -0.5x
- 6.9 × 10⁻⁶
- -6.9 × 10⁻⁶
- 0.709
- -0.709
- Equilibrium:
- x + 6.9 × 10⁻⁶
- x - 6.9 × 10⁻⁶
- x + 0.709
- x - 0.709
**Action:**
Fill in the ICE table based on provided values and calculations, then click "NEXT" to proceed. Use the various mathematical options provided to determine the correct concentrations and solve for the grams](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb67f5b4f-9f96-4f2f-93ec-c2762b2db8a1%2Fae74d24b-c5bf-42d1-9fed-02490ed1f302%2F9l6kua_processed.png&w=3840&q=75)
Transcribed Image Text:**Interactive Activity: Calculating the Grams of NH₄Br Needed**
**Problem Statement:**
How many grams of NH₄Br must be dissolved in 1.00 L of water to produce a solution with pH = 5.16? The Kb of NH₃ is equal to 1.8 × 10⁻⁵.
**Instructions:**
1. Use the ICE (Initial, Change, Equilibrium) table to determine the unknown concentration of NH₄⁺ in the solution.
2. Let x represent the initial concentration of NH₄⁺.
**Reaction:**
\[ \text{NH}_4^+(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{H}_3\text{O}^+(aq) + \text{NH}_3(aq) \]
**ICE Table Structure:**
| | NH₄⁺(aq) | + | H₂O(l) | ⇌ | H₃O⁺(aq) | + | NH₃(aq) |
|-------------------|------------|----|--------|----|----------|----|--------|
| Initial (M) | | | | | | | |
| Change (M) | | | | | | | |
| Equilibrium (M) | | | | | | | |
**Available Answer Options:**
- Variables:
- x
- 2x
- 0.5x
- Changes:
- -x
- -2x
- -0.5x
- 6.9 × 10⁻⁶
- -6.9 × 10⁻⁶
- 0.709
- -0.709
- Equilibrium:
- x + 6.9 × 10⁻⁶
- x - 6.9 × 10⁻⁶
- x + 0.709
- x - 0.709
**Action:**
Fill in the ICE table based on provided values and calculations, then click "NEXT" to proceed. Use the various mathematical options provided to determine the correct concentrations and solve for the grams
![**Transcription for Educational Website**
**Problem Statement:**
How many grams of NH₄Br must be dissolved in 1.00 L of water to produce a solution with pH = 5.16? The Kb of NH₃ is equal to 1.8 × 10⁻⁵.
**Instruction:**
Based on your ICE (Initial, Change, Equilibrium) table and the definition of Ka, set up the expression for Ka to determine the unknown. Do not combine or simplify terms.
---
**Ka Expression:**
\[ K_a = \boxed{ \phantom{placeholder} } = \boxed{ \phantom{placeholder} } \]
---
**Options Below for Selection:**
- [0]
- [1.00]
- [5.16]
- [1.8 × 10⁻⁵]
- [x]
- [2x]
- [0.5x]
- [6.9 × 10⁻⁶]
- [0.709]
- [x + 6.9 × 10⁻⁶]
- [x - 6.9 × 10⁻⁶]
- [x + 0.709]
- [x - 0.709]
- [0]
- [5.6 × 10⁻¹⁰]
- [1.8 × 10⁻¹⁹]
**RESET Button**: Resets the inputs for another attempt.
---
**Diagrams or Graphs: None**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb67f5b4f-9f96-4f2f-93ec-c2762b2db8a1%2Fae74d24b-c5bf-42d1-9fed-02490ed1f302%2Fsep1gjm_processed.png&w=3840&q=75)
Transcribed Image Text:**Transcription for Educational Website**
**Problem Statement:**
How many grams of NH₄Br must be dissolved in 1.00 L of water to produce a solution with pH = 5.16? The Kb of NH₃ is equal to 1.8 × 10⁻⁵.
**Instruction:**
Based on your ICE (Initial, Change, Equilibrium) table and the definition of Ka, set up the expression for Ka to determine the unknown. Do not combine or simplify terms.
---
**Ka Expression:**
\[ K_a = \boxed{ \phantom{placeholder} } = \boxed{ \phantom{placeholder} } \]
---
**Options Below for Selection:**
- [0]
- [1.00]
- [5.16]
- [1.8 × 10⁻⁵]
- [x]
- [2x]
- [0.5x]
- [6.9 × 10⁻⁶]
- [0.709]
- [x + 6.9 × 10⁻⁶]
- [x - 6.9 × 10⁻⁶]
- [x + 0.709]
- [x - 0.709]
- [0]
- [5.6 × 10⁻¹⁰]
- [1.8 × 10⁻¹⁹]
**RESET Button**: Resets the inputs for another attempt.
---
**Diagrams or Graphs: None**
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