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acids: 1 mol of HI is added to 1.0 L of a 0.7 M NH3 solution. bases: O ? other: I 0.05 mol of HBr is added to acids: 1.0 L of a solution that is bases: I 0.3 M in both NH3 and NH,CI. other: U

acids: 1 mol of HI is added to 1.0 L of a 0.7 M NH3 solution. bases: O ? other: I 0.05 mol of HBr is added to acids: 1.0 L of a solution that is bases: I 0.3 M in both NH3 and NH,CI. other: U

Chemistry
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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### Chemical Equilibria of Aqueous Solutions 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 \( \text{NH}_3 \) is a weak base. #### Solution 1 **Preparation:** - 1 mol of HI is added to 1.0 L of a 0.7 M \( \text{NH}_3 \) solution. **Species:** - **Acids:** - **Bases:** - **Other:** #### Solution 2 **Preparation:** - 0.05 mol of HBr is added to 1.0 L of a solution that is 0.3 M in both \( \text{NH}_3 \) and \( \text{NH}_4 \text{Cl} \). **Species:** - **Acids:** - **Bases:** - **Other:** #### Diagram Explanation The image contains a table with two separate scenarios, each detailing specific mixtures and asking for the identification of the major species present at equilibrium. Each scenario has options to classify the species into acids, bases, or other categories. Equilibrium species need to be determined based on the dissolution and reaction products of the provided compounds. For a more detailed analysis, note the following: - When HI, a strong acid, is added to \( \text{NH}_3 \), it will react with the ammonia, leading to the formation of \( \text{NH}_4^+ \) and I⁻. - Similarly, when HBr, another strong acid, is added to a solution containing \( \text{NH}_3 \) and \( \text{NH}_4 \text{Cl} \), it will shift the equilibrium towards the formation of \( \text{NH}_4^+ \) and Br⁻. ### Instructions Students are expected to complete the table by inserting the correct chemical species into the appropriate categories based on the reaction equilibria. ### Useful Reminders - \( \text{
Transcribed Image Text:### Chemical Equilibria of Aqueous Solutions 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 \( \text{NH}_3 \) is a weak base. #### Solution 1 **Preparation:** - 1 mol of HI is added to 1.0 L of a 0.7 M \( \text{NH}_3 \) solution. **Species:** - **Acids:** - **Bases:** - **Other:** #### Solution 2 **Preparation:** - 0.05 mol of HBr is added to 1.0 L of a solution that is 0.3 M in both \( \text{NH}_3 \) and \( \text{NH}_4 \text{Cl} \). **Species:** - **Acids:** - **Bases:** - **Other:** #### Diagram Explanation The image contains a table with two separate scenarios, each detailing specific mixtures and asking for the identification of the major species present at equilibrium. Each scenario has options to classify the species into acids, bases, or other categories. Equilibrium species need to be determined based on the dissolution and reaction products of the provided compounds. For a more detailed analysis, note the following: - When HI, a strong acid, is added to \( \text{NH}_3 \), it will react with the ammonia, leading to the formation of \( \text{NH}_4^+ \) and I⁻. - Similarly, when HBr, another strong acid, is added to a solution containing \( \text{NH}_3 \) and \( \text{NH}_4 \text{Cl} \), it will shift the equilibrium towards the formation of \( \text{NH}_4^+ \) and Br⁻. ### Instructions Students are expected to complete the table by inserting the correct chemical species into the appropriate categories based on the reaction equilibria. ### Useful Reminders - \( \text{
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