Using the Arrhenius concept of acids and bases, identify the Arrhenius acid and base in each of the following reactions: Drag the appropriate items to their respective bins. ▸ View Available Hint(s) Arrhenius acid NaOH(aq) H₂SO4(aq) Arrhenius base (CH3)2NH(g) HF (g) Neither 2NaOH(aq) + H₂SO4 (aq) Na₂SO4 (aq) + 2H₂O(1) (CH3)₂NH(g) + HF(g) →+(CH3)₂NH₂F(s) Reset Help
Using the Arrhenius concept of acids and bases, identify the Arrhenius acid and base in each of the following reactions: Drag the appropriate items to their respective bins. ▸ View Available Hint(s) Arrhenius acid NaOH(aq) H₂SO4(aq) Arrhenius base (CH3)2NH(g) HF (g) Neither 2NaOH(aq) + H₂SO4 (aq) Na₂SO4 (aq) + 2H₂O(1) (CH3)₂NH(g) + HF(g) →+(CH3)₂NH₂F(s) Reset Help
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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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.
Question
![**Brønsted-Lowry Concept**
Brønsted-Lowry acids are substances that can donate a proton (H⁺) to another substance; Brønsted-Lowry bases are substances that can accept a proton (H⁺).
A substance with transferable protons is an acid, such as HNO₂ in this example:
\[ \text{HNO}_2(\text{aq}) + \text{H}_2\text{O(l)} \rightleftharpoons \text{NO}_2^-(\text{aq}) + \text{H}_3\text{O}^+(\text{aq}) \]
A substance that can receive a transferable proton is a base, such as water in this example:
\[ \text{HNO}_2(\text{aq}) + \text{H}_2\text{O(l)} \rightleftharpoons \text{NO}_2^-(\text{aq}) + \text{H}_3\text{O}^+(\text{aq}) \]
One benefit of the Brønsted-Lowry concept of acids and bases is that it is not limited to aqueous solutions and can be applied to gases, liquids, and solids.
---
**Part B**
Using the Brønsted-Lowry concept of acids and bases, identify the Brønsted-Lowry acid and base in each of the following reactions:
\[ \text{HSO}_4^-(\text{aq}) + \text{H}_2\text{O(l)} \rightarrow \text{H}_2\text{SO}_4(\text{aq}) + \text{OH}^-(\text{aq}) \]
\[ (\text{CH}_3)_2\text{NH(g)} + \text{BF}_3(\text{g}) \rightarrow (\text{CH}_3)_2\text{NHB}\text{F}_3(\text{s}) \]
**Drag the appropriate items to their respective bins:**
- HSO₄⁻(aq)
- H₂O(l)
- (CH₃)₂NH(aq)
- BF₃(aq)
**Bins:**
- Brønsted-Lowry acid
- Brønsted-Lowry base
- Neither
*View Available Hint(s)*
(Buttons: Reset,](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F854eeac7-4138-4998-a76f-57a8c1b9e974%2F519fe521-4aa5-4ad2-b5b5-7d411173b553%2Fbudbjer_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Brønsted-Lowry Concept**
Brønsted-Lowry acids are substances that can donate a proton (H⁺) to another substance; Brønsted-Lowry bases are substances that can accept a proton (H⁺).
A substance with transferable protons is an acid, such as HNO₂ in this example:
\[ \text{HNO}_2(\text{aq}) + \text{H}_2\text{O(l)} \rightleftharpoons \text{NO}_2^-(\text{aq}) + \text{H}_3\text{O}^+(\text{aq}) \]
A substance that can receive a transferable proton is a base, such as water in this example:
\[ \text{HNO}_2(\text{aq}) + \text{H}_2\text{O(l)} \rightleftharpoons \text{NO}_2^-(\text{aq}) + \text{H}_3\text{O}^+(\text{aq}) \]
One benefit of the Brønsted-Lowry concept of acids and bases is that it is not limited to aqueous solutions and can be applied to gases, liquids, and solids.
---
**Part B**
Using the Brønsted-Lowry concept of acids and bases, identify the Brønsted-Lowry acid and base in each of the following reactions:
\[ \text{HSO}_4^-(\text{aq}) + \text{H}_2\text{O(l)} \rightarrow \text{H}_2\text{SO}_4(\text{aq}) + \text{OH}^-(\text{aq}) \]
\[ (\text{CH}_3)_2\text{NH(g)} + \text{BF}_3(\text{g}) \rightarrow (\text{CH}_3)_2\text{NHB}\text{F}_3(\text{s}) \]
**Drag the appropriate items to their respective bins:**
- HSO₄⁻(aq)
- H₂O(l)
- (CH₃)₂NH(aq)
- BF₃(aq)
**Bins:**
- Brønsted-Lowry acid
- Brønsted-Lowry base
- Neither
*View Available Hint(s)*
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![# Definitions of Acids and Bases
## Arrhenius Concept
Arrhenius acids are substances that, when dissolved in water, increase the concentration of the \( \text{H}^+ \) ion; Arrhenius bases are substances that, when dissolved in water, increase the concentration of the \( \text{OH}^- \) ion.
For example, a substance with an ionizable proton is an acid:
\[ \text{HNO}_2 (\text{aq}) \rightleftharpoons \text{NO}_2^- (\text{aq}) + \text{H}^+ (\text{aq}) \]
A substance that can either directly or indirectly increase hydroxide ions is a base:
\[ \text{NH}_3 (\text{aq}) + \text{H}_2\text{O(l)} \rightleftharpoons \text{NH}_4^+ (\text{aq}) + \text{OH}^- (\text{aq}) \]
However, the Arrhenius concept only applies to aqueous solutions. It does not apply to reactions in other phases, which ultimately lead to the use of other definitions for such systems.
---
## Part A
Using the Arrhenius concept of acids and bases, identify the Arrhenius acid and base in each of the following reactions:
\[ 2\text{NaOH(aq)} + \text{H}_2\text{SO}_4\text{(aq)} \rightarrow \text{Na}_2\text{SO}_4\text{(aq)} + 2\text{H}_2\text{O(l)} \]
\[ (\text{CH}_3)_2\text{NH(g)} + \text{HF(g)} \rightarrow (\text{CH}_3)_2\text{NH}_2\text{F(s)} \]
### Instructions
Drag the appropriate items to their respective bins:
- **Arrhenius Acid:**
- **Arrhenius Base:**
- **Neither:**
### Available Options:
- \(\text{NaOH(aq)}\)
- \(\text{H}_2\text{SO}_4\text{(aq)}\)
- \(\text{(CH}_3)_2\text{NH(g)}\)
- \(\text{HF(g)}\)
### Sorting Area
- **Arrhenius Acid:**
-](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F854eeac7-4138-4998-a76f-57a8c1b9e974%2F519fe521-4aa5-4ad2-b5b5-7d411173b553%2Fir0s5hd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:# Definitions of Acids and Bases
## Arrhenius Concept
Arrhenius acids are substances that, when dissolved in water, increase the concentration of the \( \text{H}^+ \) ion; Arrhenius bases are substances that, when dissolved in water, increase the concentration of the \( \text{OH}^- \) ion.
For example, a substance with an ionizable proton is an acid:
\[ \text{HNO}_2 (\text{aq}) \rightleftharpoons \text{NO}_2^- (\text{aq}) + \text{H}^+ (\text{aq}) \]
A substance that can either directly or indirectly increase hydroxide ions is a base:
\[ \text{NH}_3 (\text{aq}) + \text{H}_2\text{O(l)} \rightleftharpoons \text{NH}_4^+ (\text{aq}) + \text{OH}^- (\text{aq}) \]
However, the Arrhenius concept only applies to aqueous solutions. It does not apply to reactions in other phases, which ultimately lead to the use of other definitions for such systems.
---
## Part A
Using the Arrhenius concept of acids and bases, identify the Arrhenius acid and base in each of the following reactions:
\[ 2\text{NaOH(aq)} + \text{H}_2\text{SO}_4\text{(aq)} \rightarrow \text{Na}_2\text{SO}_4\text{(aq)} + 2\text{H}_2\text{O(l)} \]
\[ (\text{CH}_3)_2\text{NH(g)} + \text{HF(g)} \rightarrow (\text{CH}_3)_2\text{NH}_2\text{F(s)} \]
### Instructions
Drag the appropriate items to their respective bins:
- **Arrhenius Acid:**
- **Arrhenius Base:**
- **Neither:**
### Available Options:
- \(\text{NaOH(aq)}\)
- \(\text{H}_2\text{SO}_4\text{(aq)}\)
- \(\text{(CH}_3)_2\text{NH(g)}\)
- \(\text{HF(g)}\)
### Sorting Area
- **Arrhenius Acid:**
-
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Substances that bond with H+ when dissolved in water are known as?
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