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CHE 110 Chapter Notes - Chapter 4: Ionic Compound, Chemical Equation, Electrolyte

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azuremammoth471
8 Jan 2019
School
Quinnipiac University
Department
Chemistry
Course
CHE 110
Professor
All

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Document Summary

Arrhenius proposed the ionic theory of solutions to account for the electrical conductivity of water. Proposed that certain substances produce freely moving ions when they dissolve in water. These ions conduct electric current in an aqueous solution. Aqueous solutions: solutions in which water is the dissolving medium. Electrolyte: a substance that dissolves in water to gove an electrically conducting solution. Non-electrolyte: a substance that dissolves in water to give a non-conducting or very poorly conducting solution. Strong electrons: compounds that dissociate (split apart) into ions to a large (70-100%) extent when dissolved in water. Weak electrolytes: compounds that dissociate (split apart) to only a small extent when dissolved in water. Compound dissolves to give a relatively small % of ions. Solubility: ability of a substance to dissolve in water. Can be electrolytes (form conducting solutions) or non electrolytes (form non-conducting solutions) Insoluble: limited solubility in water (typically <0. 01 mol/l)

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Related Questions

What distinguishes (on an atomic/molecular level) electrolytes from non-electrolytes?
i. Ability to conduct electricity
ii. Ionic compounds dissociate into ions
iii. Substance that dissolves in water to yield a solution that conducts electricity
iv. Molecular compounds ionize into ions
v. Acids and bases are the 2 types of molecular compounds which are electrolytes
a) i, ii, iii, and v only
b) all of i, ii, iii, iv, and v
c) i only
d) i, ii, iii, and iv only
e) i and ii only

When an ionic solid dissolves in water, water molecules attract theions causing them to dissociate of come apart. The resultingdissolved ions are electrically charged particles that allow thesolution to conduct electricity. The following chemical equationsrepresent this phenomenon: NaCl (s) = Na+ (aq) + Cl- (aq)
How do I write a similar balanced chemical equation for theseelectrolyte:
NaCl HCN HCl
Na2CO3
NaHCO
NH4Cl
NH3

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.