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CHM 101 Lecture Notes - Lecture 4: Kinetic Theory Of Gases, Ionic Compound, Solubility Table

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ivorytrout555
27 Sep 2017
School
UNC
Department
Chemistry
Course
CHM 101
Professor
Dr.Jones

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Document Summary

Types of solutes: strong electrolyte, weak electrolyte, nonelectrolyte. Strong electrolyte: dissociates 100% into ions as it dissolves. Salts (ionic compounds), strong acids, and strong bases are all strong electrolytes. Weak electrolyte: dissociates partially into ions as it dissolves. Weak acids and weak bases are weak electrolytes. Nonelectrolytes: does not dissociate at all as it dissolves. Strong acids and strong bases: acid - increases hydrogen ion (h3o+) concentration in water base - increases oh concentration in water strong acids - dissociate 100% in water acid. How to name acids (works for strong and weak acids): Add prefix hydro to anion name, drop last syllable of anion name and add ic and the word acid. Oxyanion containing acids (h is actually attached to an oxygen): Drop last syllable of oxyanion name and add ic acid if anion ending is ate; add ous acid if anion name ends in ite.

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Related Questions


The Behavior of Substances in Water

Part 1:

  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.
  2. 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.
  3. 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.
  4. Hydrochloric acid, HCl, is a molecular compound that is a strong electrolyte. Write the chemical reaction of HCl with water.
  5. Compare the ammonia reaction with that of hydrochloric acid. Why are both of these substances considered electrolytes?
  6. Explain why HCl is a strong electrolyte and ammonia is a weak electrolyte.
  7. Classify each of the following substances as either ionic or molecular:
  • KCl
  • NH3
  • CO2
  • MgBr2
  • HCl
  • Ca(OH)2
  • PbS
  • HC2H3O2  
  1. For those compounds above that, you classified as ionic, use the solubility rules to determine which are soluble.
  2. 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.
  3. 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?
  4. How would you classify the soluble ionic compounds: strong electrolyte, weak electrolyte, or nonelectrolyte? Explain your answer.
  5. 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
  6. 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)

  1. 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.
  2. 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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