1. HIO3 is generally considered a weak acid when the solvent is water, but is a strong acid when dissolved in acetic acid. Using just a few sentences, explain why this is so 2. A recent report described the rainwater run-off from a strip mining operation as having a pH of −1.2. Using just a few sentences, describe what is occurring.

OneClass: 1. HIO3 is generally considered a weak acid when the solvent is water, but is a strong acid...

Just need answers 1-10. As you can see I attempted them but want to make sure on everything. I believe the odor was odorless but I'm not sure? If aspirin was created would we expect vinegar smell due to acetic acid?

4. Collect the crystals using vacuum filtration. Turn the vacuum off temporarily, pour just enough COLD water to thoroughly wet the crystals, and then turn the vacuum on. Let the vacuum draw air through the crystals for 2 minutes, making certain that the seal with the rubber ring is a good one. Place a small stals on a clean watch glass and spread them thinly to facilitate drying. Using a marker rme on the watch glass and heat the crystals for 15 minutes in an oven set at a temperature of70-80 â Determine the melting point of both your dried aspirin product and pure salicylic acid. Refer to Appendix 4 for instructions on how to take a melting point. *Pure aspirin melts at 135â and pure salicylic acid melts at 156-158 â DATA SHEET/ Questions I. Record the experimental melting ranges for your recrystallized aspirin and the starting material, salicylic acid Recrystallized aspirin Salicylic acid 2. A small melting range usually indicates that: a) The compound generally has a high melting point. 6) The compound has few impurities. c) The compound is highly impure d) The compound is likely to be soluble in water e) The compound is likely to be very unreactive. f) The compound will be difficult to recrystallize. 3. Describe the appearance of your final, recrystallized product. 4. Does the aspirin have a very strong odor, suggesting that it is a very volatile substance? 5. If all of the 2.0 g of the salicylic acid that you started with was converted to aspirin and 100% of the aspirin was recovered, the expected yield of aspirin would be 2.6 g. The isolated yield is always less than this because: (choose all that are appropriate.) Water is trapped inside the crystals. A substantial amount of the aspirin evaporates. Some aspirin remains dissolved in the solvent from the first filtration. Some aspirin remains dissolved in the solvent from the recrystallization. e) The reaction used to create the aspirin does not go to completion. 1 The acetic acid formed in the reaction adversely affects the yield of aspirin. Chem 162-Aspirin tab

Just need answers 1-10. As you can see I attempted them but want to make sure on everything. I believe the odor was odorless but I'm not sure? If aspirin was created would we expect vinegar smell due to acetic acid?

4. Collect the crystals using vacuum filtration. Turn the vacuum off temporarily, pour just enough COLD water to thoroughly wet the crystals, and then turn the vacuum on. Let the vacuum draw air through the crystals for 2 minutes, making certain that the seal with the rubber ring is a good one. Place a small stals on a clean watch glass and spread them thinly to facilitate drying. Using a marker rme on the watch glass and heat the crystals for 15 minutes in an oven set at a temperature of70-80 â Determine the melting point of both your dried aspirin product and pure salicylic acid. Refer to Appendix 4 for instructions on how to take a melting point. *Pure aspirin melts at 135â and pure salicylic acid melts at 156-158 â DATA SHEET/ Questions I. Record the experimental melting ranges for your recrystallized aspirin and the starting material, salicylic acid Recrystallized aspirin Salicylic acid 2. A small melting range usually indicates that: a) The compound generally has a high melting point. 6) The compound has few impurities. c) The compound is highly impure d) The compound is likely to be soluble in water e) The compound is likely to be very unreactive. f) The compound will be difficult to recrystallize. 3. Describe the appearance of your final, recrystallized product. 4. Does the aspirin have a very strong odor, suggesting that it is a very volatile substance? 5. If all of the 2.0 g of the salicylic acid that you started with was converted to aspirin and 100% of the aspirin was recovered, the expected yield of aspirin would be 2.6 g. The isolated yield is always less than this because: (choose all that are appropriate.) Water is trapped inside the crystals. A substantial amount of the aspirin evaporates. Some aspirin remains dissolved in the solvent from the first filtration. Some aspirin remains dissolved in the solvent from the recrystallization. e) The reaction used to create the aspirin does not go to completion. 1 The acetic acid formed in the reaction adversely affects the yield of aspirin. Chem 162-Aspirin tab

The Behavior of Substances in Water

Part 1:

Ammonia, NH₃, is a weak electrolyte. It forms ions in solution by reacting with water molecules to form the ammonium ion and hydroxide ion. Write the balanced chemical reaction for this process, including state symbols.
From everyday experience, you are probably aware that table sugar (sucrose), C₁₂H₂₂O₁₁, is soluble in water. When sucrose dissolves in water, it doesn’t form ions through any reaction with water. It just dissolves without forming ions, so it is a nonelectrolyte. Write the chemical equation for the dissolving of sucrose in water.
Both NH₃ and C₁₂H₂₂O₁₁ are soluble molecular compounds, yet they behave differently in an aqueous solution. Briefly explain why one is a weak electrolyte and the other is a nonelectrolyte.
Hydrochloric acid, HCl, is a molecular compound that is a strong electrolyte. Write the chemical reaction of HCl with water.
Compare the ammonia reaction with that of hydrochloric acid. Why are both of these substances considered electrolytes?
Explain why HCl is a strong electrolyte and ammonia is a weak electrolyte.
Classify each of the following substances as either ionic or molecular:

KCl
NH₃
CO₂
MgBr₂
HCl
Ca(OH)₂
PbS
HC₂H₃O₂

For those compounds above that, you classified as ionic, use the solubility rules to determine which are soluble.
The majority of ionic substances are solids at room temperature. Describe what you would observe if you placed a soluble ionic compound and an insoluble ionic compound in separate beakers of water.
Write the chemical equation(s), including state symbols, for what happens when each soluble ionic compound that you identified above is placed in water. Are these substances reacting with water when they are added to water?
How would you classify the soluble ionic compounds: strong electrolyte, weak electrolyte, or nonelectrolyte? Explain your answer.
Sodium chloride, NaCl, is a strong electrolyte, as is hydroiodic acid, HI. Write the chemical equations for what happens when these substances are added to water. m
Are NaCl and HI strong electrolytes because they have similar behavior in an aqueous solution? If not, describe, using words and equations, the different chemical process that takes place in each case.

Part 2:

You have two hypothetical molecular compounds, AX and AY. AX is a strong electrolyte and AY is a weak electrolyte. The compounds undergo the following chemical reactions when added to water.

AX (aq) + H₂O (l) → AH₂O⁺ (aq) + X⁻ (aq)

AY (aq) + H₂O (l) → AH₂O⁺ (aq) + Y⁻ (aq)

Explain how the relative amounts of AX ( aq ) and AY ( aq ) would compare if you had a beaker of water with AX and a beaker of water with AY.
How would the relative amounts of X⁻ ( aq) and Y⁻ ( aq) in the two beakers compare? Be sure to explain your answer.

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