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Write the chemical formulas of the species that will act as formulas of the species that will act as neither acids nor bases in th You will find it useful to keep in mind that HF is a weak acid. acids: O 0.55 mol of NAOH is added to 1.0 L of a 1.3 M HF bases: O OH f solution. other: U Na + acids: O HF 0.54 mol of HNO, is added 3. to 1.0 L of a solution that is bases: 1.4 M in both HF and NaF. other: U NO2, Na

Write the chemical formulas of the species that will act as formulas of the species that will act as neither acids nor bases in th You will find it useful to keep in mind that HF is a weak acid. acids: O 0.55 mol of NAOH is added to 1.0 L of a 1.3 M HF bases: O OH f solution. other: U Na + acids: O HF 0.54 mol of HNO, is added 3. to 1.0 L of a solution that is bases: 1.4 M in both HF and NaF. other: U NO2, Na

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter14: Acids And Bases
Section: Chapter Questions
Problem 107QRT: When all the water is evaporated from a sodium hydroxide solution, solid sodium hydroxide is...
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**Title: Understanding Acid-Base Equilibria with HF Solutions** When studying acid-base reactions, it's essential to identify which species act as acids, bases, or neither. Consider the following scenarios involving hydrofluoric acid (HF), a weak acid. **Scenario 1: Reaction with NaOH** *A total of 0.55 mol of NaOH is added to 1.0 L of a 1.3 M HF solution.* - In this scenario, identify the species: - **Acids:** (No acids identified here, as HF reacts completely with NaOH) - **Bases:** \( \text{OH}^- \), \( \text{F}^- \) - **Other:** \( \text{Na}^+ \) **Scenario 2: Reaction with HNO3** *A total of 0.54 mol of HNO3 is added to 1.0 L of a solution that is 1.4 M in both HF and NaF.* - In this scenario, identify the species: - **Acids:** \( \text{HF} \) - **Bases:** \( \text{F}^- \) - **Other:** \( \text{NO}_3^- \), \( \text{Na}^+ \) **Equilibrium and Reaction Calculations:** *Reaction: \( \text{HF} + \text{NaOH} \rightarrow \text{NaF} + \text{H}_2\text{O} \)* - Initial moles: - HF: 1.3 mol - NaOH: 0.55 mol - Change during reaction: - HF: -1.3 mol (complete reaction) - NaOH: -1.3 mol (complete reaction) - NaF: +1.3 mol - End of reaction: - HF: 0 mol - NaOH: -0.75 mol (excess) - NaF: 1.3 mol This exercise helps illustrate the concepts of acid-base interactions and the dynamic nature of chemical equilibria, particularly when dealing with a weak acid like HF.
Transcribed Image Text:**Title: Understanding Acid-Base Equilibria with HF Solutions** When studying acid-base reactions, it's essential to identify which species act as acids, bases, or neither. Consider the following scenarios involving hydrofluoric acid (HF), a weak acid. **Scenario 1: Reaction with NaOH** *A total of 0.55 mol of NaOH is added to 1.0 L of a 1.3 M HF solution.* - In this scenario, identify the species: - **Acids:** (No acids identified here, as HF reacts completely with NaOH) - **Bases:** \( \text{OH}^- \), \( \text{F}^- \) - **Other:** \( \text{Na}^+ \) **Scenario 2: Reaction with HNO3** *A total of 0.54 mol of HNO3 is added to 1.0 L of a solution that is 1.4 M in both HF and NaF.* - In this scenario, identify the species: - **Acids:** \( \text{HF} \) - **Bases:** \( \text{F}^- \) - **Other:** \( \text{NO}_3^- \), \( \text{Na}^+ \) **Equilibrium and Reaction Calculations:** *Reaction: \( \text{HF} + \text{NaOH} \rightarrow \text{NaF} + \text{H}_2\text{O} \)* - Initial moles: - HF: 1.3 mol - NaOH: 0.55 mol - Change during reaction: - HF: -1.3 mol (complete reaction) - NaOH: -1.3 mol (complete reaction) - NaF: +1.3 mol - End of reaction: - HF: 0 mol - NaOH: -0.75 mol (excess) - NaF: 1.3 mol This exercise helps illustrate the concepts of acid-base interactions and the dynamic nature of chemical equilibria, particularly when dealing with a weak acid like HF.
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