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
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![**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)
![**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)
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