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Ch 17-18 Review

Ch 17-18 Review. 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. AgNO 3 + NaCl  NaNO 3 + AgCl (s) Write a complete ionic equation.

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Ch 17-18 Review

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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. AgNO3 + NaCl NaNO3 + AgCl(s) • Write a complete ionic equation. Ag+ + NO3- + Na+ + Cl- AgCl(s) + Na+ + NO3- • Write a net-ionic equation Ag+ + Cl- AgCl(s)

  3. 2. Define the following: a. Hydrogen bonds – a weak bond between hydrogen and an element with a higher electronegativity b. Hygroscopic – salts and other compounds that remove moisture from the air c. Desiccant – drying agents d. Deliquescent – remove water from the air to dissolve completely to form solutions e. Efflorescent – process at which the hydrate losses water of hydration

  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) will dissolve in water b. Na2SO4 will dissolve in water c. Methane (CH4) will dissolve in gas d. KClwill dissolve in water

  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 a, b • Heterogeneous mixture b, c • Particle size less than 1.0nm a • Particles can be filtered out c • Demonstrates the Tyndall Effect b, c • Particles are invisible to the unaided eye a, b • Homogeneous milk b • Salt water a • Jelly b

  6. Name and distinguish between the two components of a solution. solute – substance being dissolved solvent – substance doing the dissolving

  7. Explain the difference between miscible and immiscible. Provide examples of each. miscible – 2 liquids that will dissolve in each other Ex. Water and vinegar immiscible – 2 liquids that will not dissolve in each other Ex. Water and oil

  8. Explain the difference between an unsaturated, saturated and supersaturated solution. Unsaturated – contains less than the maximum amount of solute dissolved at a given temperature Saturated – contains the maximum amount of solute dissolved at a given temp. Supersaturated – contains more than the maximum amount of solute at a given temp

  9. What mass of KNO3 can be dissolved into100 g of water at 20oC. (use Figure 18.4 on page 504) About 27 grams

  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 atm0.016 g / L b. 1.80 atm0.047 g / L

  11. 10. Calculate the molarity (M) of each solution: • 1.0 mol KCl in 750 mL of solution 1.3 M • 0.50 mol MgCl2 in 1.5 L of solution 0.33 M

  12. 11. Calculate the moles and grams of solute in each solution: • 1.0 L of 0.50M NaCl0.50 mol and 29 grams • 5.0 x 102mL of 2.0M KNO31.0 mol and 100. grams

  13. 12. What is the concentration (in % m/v) of the following solutions: a. 20.0 g KCl in 0.60 L of solution 3.3% • 32 g NaNO3 in 2.0 L of solution 1.6% 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 -4.46 oC b. 0.060 mol MgSO4 in 100 g H2O -1.1 oC

  15. 14. Determine the freezing points of each 0.20m aqueous solutions. (use the Kf for water) • K2SO4-1.1 oC • CsNO3 -0.74 oC • Al(NO3)3 -1.5 oC

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