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Chemistry Review of Solutions and Solvents

This review covers topics such as chemical reactions of solutions, types of bonding, solvent polarities, solution components, solubility, molarity calculations, and freezing point determinations.

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Chemistry Review of Solutions and Solvents

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  1. Ch 17-18 Review

  2. 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

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

  4. 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

  5. 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

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

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

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

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

  10. 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

  11. 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

  12. 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

  13. 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)

  14. 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

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

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