Indicate whether each of the following compounds will gave an acidic, basic or neutral solution when dissolved in water. Clear All ammonium iodide barium nitrite sodium iodide calcium bromide The pH will be less than 7. The pH will be approximately equal to 7. The pH will be greater than 7.
Indicate whether each of the following compounds will gave an acidic, basic or neutral solution when dissolved in water. Clear All ammonium iodide barium nitrite sodium iodide calcium bromide The pH will be less than 7. The pH will be approximately equal to 7. The pH will be greater than 7.
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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Indicate whether each of the following compounds will gave an acidic, basic or neutral solution when dissolved in water.
Use the References to access important values if needed for this question.
Indicate whether each of the following compounds will gave an acidic, basic or neutral solution when dissolved in water.
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![**The pH of Aqueous Salt Solutions**
When a salt dissolves in water, it may cause the pH of the solution to change. To determine whether the resulting solution will be acidic, basic, or approximately neutral, you must examine first how the cation interacts with water, and then how the anion interacts with water.
If, by interacting with water, a weak acid or base can form, the salt changes the pH of the solution. The driving force for the reaction is the formation of the weak acid or base.
---
**Cations of weak bases are ACIDIC.** They donate H⁺ to water, making the weak base and H₃O⁺, which reduces the pH of the solution:
\[ \text{NH}_4^+ (aq) + \text{H}_2\text{O} \rightarrow \text{NH}_3(aq) + \text{H}_3\text{O}^+ (aq) \]
- *Donates H⁺*
- *Weak Base*
- *ACIDIC Solution*
---
**Cations of strong bases are NEUTRAL.** They do not interact with water:
\[ \text{Na}^+ (aq) + \text{H}_2\text{O} \rightarrow \text{No Reaction} \]
---
**Anions of weak acids are BASIC.** They accept H⁺ from water, making the weak acid and OH⁻, which increases the pH of the solution:
\[ \text{F}^- (aq) + \text{H}_2\text{O} \rightarrow \text{HF}(aq) + \text{OH}^- (aq) \]
- *Accepts H⁺*
- *Weak Acid*
- *BASIC Solution*
---
**Anions of strong acids are NEUTRAL.** They do not interact with water:
\[ \text{Cl}^- (aq) + \text{H}_2\text{O} \rightarrow \text{No Reaction} \]
---
**Most anions of polyprotic acids are BASIC,** accepting H⁺ from water, although some act as acids and donate a proton to water.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3d2b0534-65d7-4c4f-8595-adc051f2d27b%2F1a7282ef-e4e8-4be6-8821-c3faa9791eb0%2Fu78xkvt_processed.png&w=3840&q=75)
Transcribed Image Text:**The pH of Aqueous Salt Solutions**
When a salt dissolves in water, it may cause the pH of the solution to change. To determine whether the resulting solution will be acidic, basic, or approximately neutral, you must examine first how the cation interacts with water, and then how the anion interacts with water.
If, by interacting with water, a weak acid or base can form, the salt changes the pH of the solution. The driving force for the reaction is the formation of the weak acid or base.
---
**Cations of weak bases are ACIDIC.** They donate H⁺ to water, making the weak base and H₃O⁺, which reduces the pH of the solution:
\[ \text{NH}_4^+ (aq) + \text{H}_2\text{O} \rightarrow \text{NH}_3(aq) + \text{H}_3\text{O}^+ (aq) \]
- *Donates H⁺*
- *Weak Base*
- *ACIDIC Solution*
---
**Cations of strong bases are NEUTRAL.** They do not interact with water:
\[ \text{Na}^+ (aq) + \text{H}_2\text{O} \rightarrow \text{No Reaction} \]
---
**Anions of weak acids are BASIC.** They accept H⁺ from water, making the weak acid and OH⁻, which increases the pH of the solution:
\[ \text{F}^- (aq) + \text{H}_2\text{O} \rightarrow \text{HF}(aq) + \text{OH}^- (aq) \]
- *Accepts H⁺*
- *Weak Acid*
- *BASIC Solution*
---
**Anions of strong acids are NEUTRAL.** They do not interact with water:
\[ \text{Cl}^- (aq) + \text{H}_2\text{O} \rightarrow \text{No Reaction} \]
---
**Most anions of polyprotic acids are BASIC,** accepting H⁺ from water, although some act as acids and donate a proton to water.
Transcribed Image Text:**Summary - pH of Aqueous Salt Solutions**
**ACIDIC CATIONS**
1. **Cations of WEAK Bases**
- NH₄⁺ (main example in General Chemistry)
2. **Some Metal cations**
- Al³⁺, transition metal ions
**ACIDIC ANIONS**
- Some anions of polyprotic acids:
- HSO₄⁻, H₂PO₄⁻, HSO₃⁻
---
**NEUTRAL CATIONS**
- **Cations of STRONG Bases**
- Li⁺, Na⁺, K⁺
- Ca²⁺, Ba²⁺, Sr²⁺
**NEUTRAL ANIONS**
- **Anions of STRONG Acids**
- Cl⁻, Br⁻, I⁻, NO₃⁻, ClO₄⁻
---
**BASIC CATIONS**
- None (think about why)
**BASIC ANIONS**
1. **Anions of WEAK acids**
- F⁻, CH₃COO⁻, ClO⁻
- HCOO⁻, CN⁻, NO₂⁻
2. **Most anions of polyprotic acids**
- HCO₃⁻, HS⁻, HCO₃⁻, HPO₄²⁻
- CO₃²⁻, SO₄²⁻, SO₃²⁻, S²⁻, S²⁻, PO₄³⁻
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