Ch 17-18 Review

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Ch 17-18 Review
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• 1. A clear solution of silver nitrate is mixed
  with a solution of sodium chloride and a white
  precipitate forms.
• Write a balanced equation for this reaction.
• Write a complete ionic equation.
• Write a net-ionic equation

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• 2. Define the following
• a. Hydrogen bonds
• b. Hygroscopic
• c. Desiccant
• d. Deliquescent
• e. efflorescent

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• 3. Water is a polar solvent gasoline is a
  nonpolar solvent. Decide which compounds are
  more likely to dissolve in water and which are
  more likely to dissolve in gasoline?
• a. Sucrose (C12H22O11)
• b. Na2SO4
• c. Methane (CH4)
• d. KCl

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• 4. Match each term with the following
  descriptions. A description may apply to more
  than one term.
• a. True solution b. Colloid c. Suspension
• Does not settle out on standing
• Heterogeneous mixture
• Particle size less than 1.0nm
• Particles can be filtered out
• Demonstrates the Tyndall Effect
• Particles are invisible to the unaided eye
• Homogeneous milk
• Salt water
• jelly

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• 5. Name and distinguish between the town
  components of a solution.

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• 6. Explain the difference between miscible and
  immiscible. Provide examples of each.

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• 7. Explain the difference between an
  unsaturated, saturated and supersaturated
  solution.

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• 8. What mass of KNO3 can be dissolved into100 g
  of water at 20oC. (use Figure 18.4 on page 504)

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• 9. The solubility of methane, the major
  component of natural gas, in water at 20oC and
  1.00 atm of pressure is 0.026 g / L. If the
  temperature remains constant, what will be the
  solubility of this gas at the following pressure?
• a. 0.60 atm
• b. 1.80 atm

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• 10. Calculate the molarity (M) of each solution
• 1.0 mol KCl in 750 mL of solution
• 0.50 mol MgCl2 in 1.5 L of solution

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• 11. Calculate the moles and grams of solute in
  each solution
• 1.0 L of 0.50M NaCl
• 5.0 x 102 mL of 2.0M KNO3

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• 12. What is the concentration (in m/v) of the
  following solutions
• a. 20.0 g KCl in 0.60 L of solution
• 32 g NaNO3 in 2.0 L of solution
• HINT (m / v) mass / vol
• (g / mL)

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• 13. What is the freezing point of each solution?
• a. 1.40 mol Na2SO4 in 1750 g H2O
• b. 0.060 mol MgSO4 in 100 g H2O

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• 14. Determine the freezing points of each 0.20m
  aqueous solutions. (use the Kf for water)
• K2SO4
• CsNO3
• Al(NO3)3