The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH3 is a weak base. 2.3 mol of HNO3 is added to 1.0 L of a 1.4M NH3 solution. 0.3 mol of KOH is added to 1.0 L of a solution that is 0.7M in both NH3 and NH4Br. acids: bases: other: acids: bases: other: 0 0 X 0.0.... S
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH3 is a weak base. 2.3 mol of HNO3 is added to 1.0 L of a 1.4M NH3 solution. 0.3 mol of KOH is added to 1.0 L of a solution that is 0.7M in both NH3 and NH4Br. acids: bases: other: acids: bases: other: 0 0 X 0.0.... S
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Question
![**Preparation of Aqueous Solutions and Identification of Major Species at Equilibrium**
This section provides descriptions of two aqueous solutions and instructs how to identify the major species present at equilibrium. Please omit water in your analysis.
For each solution, write the chemical formulas of the species that will act as acids, bases, and those that will act as neither (other).
Note: \( NH_3 \) is a weak base and this will be relevant in your evaluations.
**Solution 1:**
- **Preparation:** 2.3 mol of \( HNO_3 \) is added to 1.0 L of a 1.4 M \( NH_3 \) solution.
- **Acids:** [ ]
- **Bases:** [ ]
- **Other:** [ ]
**Solution 2:**
- **Preparation:** 0.3 mol of \( KOH \) is added to 1.0 L of a solution that is 0.7 M in both \( NH_3 \) and \( NH_4Br \).
- **Acids:** [ ]
- **Bases:** [ ]
- **Other:** [ ]
Please refer to the relevant chemical principles to complete the analysis.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa60cc6ce-11de-444a-af29-e9eb1b50e640%2F69561402-4c25-435f-a6bc-350f6f57b8cf%2F5czfoci_processed.png&w=3840&q=75)
Transcribed Image Text:**Preparation of Aqueous Solutions and Identification of Major Species at Equilibrium**
This section provides descriptions of two aqueous solutions and instructs how to identify the major species present at equilibrium. Please omit water in your analysis.
For each solution, write the chemical formulas of the species that will act as acids, bases, and those that will act as neither (other).
Note: \( NH_3 \) is a weak base and this will be relevant in your evaluations.
**Solution 1:**
- **Preparation:** 2.3 mol of \( HNO_3 \) is added to 1.0 L of a 1.4 M \( NH_3 \) solution.
- **Acids:** [ ]
- **Bases:** [ ]
- **Other:** [ ]
**Solution 2:**
- **Preparation:** 0.3 mol of \( KOH \) is added to 1.0 L of a solution that is 0.7 M in both \( NH_3 \) and \( NH_4Br \).
- **Acids:** [ ]
- **Bases:** [ ]
- **Other:** [ ]
Please refer to the relevant chemical principles to complete the analysis.
Expert Solution
Step 1: Determine the major species remaining after add acid and base to the given solutions:
Given,
The solutions are:
| 2.3 mol of HNO3 is added to 1.0 L of a 1.4 M NH3 solution. | acids: bases: other: |
| 0.3 mol KOH is added to 1.0 L of a solution that is 0.7 M in both NH3 and NH4Br. | acids: bases: other: |
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