2. Silver chloride is not very water soluble. The reaction by which it goes into solution hydroxide solution are added to the solution it turns yellow. Explain these observations hydrochloric acid are added the solution turns red. When several drops of sodium When methyl orange is added to water, the solution turns yellow. When a few drops of 1. Methyl orange, HMO, is an acid base indicator which ionizes according to this NAME equation: HMO(aq) Red H"aq) MO(aq) yellow in terms of LeChatelier's Principle. is: AGCI(s) Agl (aq) + CI"(aq) Suppose a saturated solution of silver chloride were present. What would happen is you added a few milliliters of HCl solution? Why? Why? What would happen if you added a few milliliters of silver nitrate solution? If this reaction is known to be endothermic, what would happen if the solution were heated? What if the solution were cooled?
2. Silver chloride is not very water soluble. The reaction by which it goes into solution hydroxide solution are added to the solution it turns yellow. Explain these observations hydrochloric acid are added the solution turns red. When several drops of sodium When methyl orange is added to water, the solution turns yellow. When a few drops of 1. Methyl orange, HMO, is an acid base indicator which ionizes according to this NAME equation: HMO(aq) Red H"aq) MO(aq) yellow in terms of LeChatelier's Principle. is: AGCI(s) Agl (aq) + CI"(aq) Suppose a saturated solution of silver chloride were present. What would happen is you added a few milliliters of HCl solution? Why? Why? What would happen if you added a few milliliters of silver nitrate solution? If this reaction is known to be endothermic, what would happen if the solution were heated? What if the solution were cooled?
Chemistry
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Methyl Orange and Silver Chloride Reactions**
1. **Methyl Orange Indicator Reaction:**
Methyl orange, HMO, is an acid-base indicator which ionizes according to the following equation:
\[
\text{HMO}_{(aq)} \rightleftharpoons \text{H}^+_{(aq)} + \text{MO}^-_{(aq)}
\]
- **Red** when HMO
- **Yellow** when MO
- **Observations:**
- When methyl orange is added to water, the solution turns yellow.
- Adding a few drops of hydrochloric acid turns the solution red.
- Adding several drops of sodium hydroxide solution returns the solution to yellow.
- **Explanation using Le Chatelier's Principle:**
- The color change is due to equilibrium shifts. Adding acid increases \([\text{H}^+]\), shifting equilibrium left, turning the solution red.
- Adding a base decreases \([\text{H}^+]\), shifting equilibrium right, and turning back to yellow.
2. **Silver Chloride Solubility Reaction:**
Silver chloride is not very water soluble. The dissolution reaction is:
\[
\text{AgCl}_{(s)} \rightleftharpoons \text{Ag}^+_{(aq)} + \text{Cl}^-_{(aq)}
\]
- **Question:**
- What happens if a few milliliters of HCl solution are added to a saturated solution of silver chloride? Why?
- **Explanation:**
- The addition of \(\text{Cl}^-\) ions from HCl increases the concentration of chloride ions, shifting equilibrium left, causing precipitation of \(\text{AgCl}\).
- **Question:**
- What happens if a few milliliters of silver nitrate solution are added? Why?
- **Explanation:**
- The addition of \(\text{Ag}^+\) from silver nitrate increases silver ion concentration, shifting equilibrium left, causing \(\text{AgCl}\) to precipitate.
- **Endothermic Reaction Points:**
- If the reaction is endothermic, heating the solution will shift the equilibrium right, increasing solubility.
- Cooling the solution will shift equilibrium left, decreasing solubility](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F055086f6-4d26-404b-b10d-4e78791428d4%2Fd4e055b6-60b3-446c-ae55-f371f015f43a%2Ftocfv1_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Methyl Orange and Silver Chloride Reactions**
1. **Methyl Orange Indicator Reaction:**
Methyl orange, HMO, is an acid-base indicator which ionizes according to the following equation:
\[
\text{HMO}_{(aq)} \rightleftharpoons \text{H}^+_{(aq)} + \text{MO}^-_{(aq)}
\]
- **Red** when HMO
- **Yellow** when MO
- **Observations:**
- When methyl orange is added to water, the solution turns yellow.
- Adding a few drops of hydrochloric acid turns the solution red.
- Adding several drops of sodium hydroxide solution returns the solution to yellow.
- **Explanation using Le Chatelier's Principle:**
- The color change is due to equilibrium shifts. Adding acid increases \([\text{H}^+]\), shifting equilibrium left, turning the solution red.
- Adding a base decreases \([\text{H}^+]\), shifting equilibrium right, and turning back to yellow.
2. **Silver Chloride Solubility Reaction:**
Silver chloride is not very water soluble. The dissolution reaction is:
\[
\text{AgCl}_{(s)} \rightleftharpoons \text{Ag}^+_{(aq)} + \text{Cl}^-_{(aq)}
\]
- **Question:**
- What happens if a few milliliters of HCl solution are added to a saturated solution of silver chloride? Why?
- **Explanation:**
- The addition of \(\text{Cl}^-\) ions from HCl increases the concentration of chloride ions, shifting equilibrium left, causing precipitation of \(\text{AgCl}\).
- **Question:**
- What happens if a few milliliters of silver nitrate solution are added? Why?
- **Explanation:**
- The addition of \(\text{Ag}^+\) from silver nitrate increases silver ion concentration, shifting equilibrium left, causing \(\text{AgCl}\) to precipitate.
- **Endothermic Reaction Points:**
- If the reaction is endothermic, heating the solution will shift the equilibrium right, increasing solubility.
- Cooling the solution will shift equilibrium left, decreasing solubility
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