Write obervation and the complete molecular equation for each reaction. Identify each reaction as redox or non-redox. A1: Mg will burn with a bright color and turn into ash. redox or non-redox: Observation: Equation: A2: Dissolving collected ash from Al in water and then adding phenolpthalein to the solution result in a pink color solution. redox or non-redox: Observation: Equation:
Write obervation and the complete molecular equation for each reaction. Identify each reaction as redox or non-redox. A1: Mg will burn with a bright color and turn into ash. redox or non-redox: Observation: Equation: A2: Dissolving collected ash from Al in water and then adding phenolpthalein to the solution result in a pink color solution. redox or non-redox: Observation: Equation:
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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Question
Write obervation and the complete molecular equation for each reaction. Identify each reaction as redox or non-redox.
A1: Mg will burn with a bright color and turn into ash.
redox or non-redox:
Observation:
Equation:
A2: Dissolving collected ash from Al in water and then adding phenolpthalein to the solution result in a pink color solution.
redox or non-redox:
Observation:
Equation:
Transcribed Image Text:## Solubility Table
The table provides information on the solubility of various compounds in water and acids. It categorizes compounds based on their solubility properties with a shorthand code:
- **W**: Soluble in water
- **A**: Insoluble in water, soluble in acids
- **w**: Insoluble in water, slightly soluble in acids
- **d**: Decompose in water
- **—**: No data available
### Table Content
- **Cations (down the left)**:
- Zr⁴⁺, Sr²⁺, Na⁺, Ag⁺, K⁺, Ni²⁺, Hg²⁺, Hg²⁺, Mg²⁺, Fe²⁺, Fe³⁺, H⁺, Cu²⁺, Co²⁺, Ca²⁺, Ba²⁺, NH₄⁺, Al³⁺
- **Anions (across the top)**:
- CH₃COO⁻, Br⁻, CO₃²⁻, Cl⁻, ClO₃⁻, OH⁻, NO₃⁻, PO₄³⁻, SO₄²⁻, S²⁻
### Examples
- **Ag⁺ / Cl⁻**: A (Insoluble in water, soluble in acids)
- **Na⁺ / SO₄²⁻**: W (Soluble in water)
- **Ba²⁺ / PO₄³⁻**: A (Insoluble in water, soluble in acids)
### Observations
The table displays solubility patterns that are useful for predicting reactions. For example, most sulfates apart from Ba²⁺ are soluble in water (W), whereas carbonates tend to be insoluble or have reduced solubility (A or w).
This table is invaluable for students and professionals dealing with chemical reactions in aqueous solutions. Understanding solubility can help predict precipitate formation and other reaction outcomes.
![**Part I: Metathetical Reactions**
Metathetical reactions, also known as double-replacement reactions, occur when two compounds exchange ions in an aqueous solution. The general formula is:
\[ AC + BD \rightarrow AD + BC \]
### A. Precipitation Reactions
In this type of reaction, a precipitate is formed. The presence of a precipitate can be predicted using solubility rules or a solubility chart. In these reactions, all soluble compounds are considered dissociated into their ions. The ions that do not participate in forming the precipitate are known as "spectator ions."
**Examples:**
1. \[ \text{AgNO}_3 \, (\text{aq}) + \text{NaCl} \, (\text{aq}) \rightarrow \text{AgCl} \, (\text{s}) \downarrow + \text{NaNO}_3 \, (\text{aq}) \]
2. \[ \text{Cd(NO}_3)_2 \, (\text{aq}) + \text{(NH}_4)_2\text{S} \, (\text{aq}) \rightarrow \text{CdS} \, (\text{s}) \downarrow + \text{NH}_4\text{NO}_3 \, (\text{aq}) \]
**Procedures:**
Perform each of the following reactions, write your observations in your notebook, and indicate the formation of any precipitate:
1. Add a dropperful of 0.1 M calcium nitrate to a test tube. Add a dropperful of 0.1 M sodium carbonate.
2. Add a dropperful of 0.1 M magnesium sulfate to a test tube. Add a dropperful of 0.1 M sodium hydroxide.
3. Add a dropperful of 0.1 M sodium nitrate in a test tube. Add a dropperful of 0.1 M potassium chloride.
### B. Acid-Base Reactions
[Text in this section is cut off from the image.]
### Important Note:
Handle all acids and caustic chemicals under a fume hood.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F81ac168b-024d-494f-99de-3f3384ea3f4e%2F9752117c-ccee-46cf-99ed-a1f657f82770%2Fzvwmko_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Part I: Metathetical Reactions**
Metathetical reactions, also known as double-replacement reactions, occur when two compounds exchange ions in an aqueous solution. The general formula is:
\[ AC + BD \rightarrow AD + BC \]
### A. Precipitation Reactions
In this type of reaction, a precipitate is formed. The presence of a precipitate can be predicted using solubility rules or a solubility chart. In these reactions, all soluble compounds are considered dissociated into their ions. The ions that do not participate in forming the precipitate are known as "spectator ions."
**Examples:**
1. \[ \text{AgNO}_3 \, (\text{aq}) + \text{NaCl} \, (\text{aq}) \rightarrow \text{AgCl} \, (\text{s}) \downarrow + \text{NaNO}_3 \, (\text{aq}) \]
2. \[ \text{Cd(NO}_3)_2 \, (\text{aq}) + \text{(NH}_4)_2\text{S} \, (\text{aq}) \rightarrow \text{CdS} \, (\text{s}) \downarrow + \text{NH}_4\text{NO}_3 \, (\text{aq}) \]
**Procedures:**
Perform each of the following reactions, write your observations in your notebook, and indicate the formation of any precipitate:
1. Add a dropperful of 0.1 M calcium nitrate to a test tube. Add a dropperful of 0.1 M sodium carbonate.
2. Add a dropperful of 0.1 M magnesium sulfate to a test tube. Add a dropperful of 0.1 M sodium hydroxide.
3. Add a dropperful of 0.1 M sodium nitrate in a test tube. Add a dropperful of 0.1 M potassium chloride.
### B. Acid-Base Reactions
[Text in this section is cut off from the image.]
### Important Note:
Handle all acids and caustic chemicals under a fume hood.
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