Honors Chemistry Unit 9 Study Guide
1. Find the molarity (M) of a solution that has 13.0 mol of solute in 4.0 liters of solution.
2. Which mass of solute is required to prepare 250.0 mL of 0.600 M Sodium Chloride, NaCl?
3. What is happens to the number of solute particles during dilution? What about the number of solvent particles?
4. What volume (mL) of 13.5 M H2SO4 would be needed to prepare 225 mL of 2.50 M H2SO4?
5. Why does naphthalene (C10H8) dissolve in oil but not water?
6. Describe the following types of solutions: saturated, unsaturated, and supersaturated
Use the solubility curve to answer questions 7-9
7. At what temperature do lead nitrate (Pb(NO3)2) and potassium nitrate (KNO3) have the same solubility?
8. Which substances decrease in solubility as temperature increases?
9. A saturated solution of K2Cr2O7 is dissolved in 100 g of water at 80°C. If the solution is cooled to 50°C, how many grams of precipitate will form?
Use the graph to answer questions #10-12
10. On the reaction rate graph above, label the reactants, products, and activation energy.
11. Is this reaction endothermic or exothermic?
12. Draw a new curve that shows how a catalyst would affect this reaction.
13. In Beaker A, 200mL of 0.5 M HCl is added to 2 grams of powdered zinc. In Beaker B, 200mL of 0.5 M HCl is added to a 2 gram solid chunk of zinc. Which beaker will react faster and why?
Use the graph to answer questions 14 and 15
14. Explain the difference in the curves for data set 1 and 2.
15. Which trend line would indicate a reaction with increased surface area, increased concentration and increased temperature?
16. Write the equilibrium expression for the following reaction: PCl5 (g) ↔ PCl3 (g) + Cl2 (g)
17. Write the equilibrium expression for the following reaction: CaCl2(s) ↔ Ca2+ (aq) + 2Cl- (aq)
18. For the following reaction at equilibrium, the concentration of water vapor is 0.80 M, the concentration of chlorine is 1.2 M, the concentration of oxygen is 0.25 M, and the concentration of HCl is 0.50 M. Calculate Keq.
4 HCl (g) + O2 (g) ↔ 2 H2O (g) + 2 Cl2 (g)
Use the following reversible reaction for problems 19-23: 2 SO2 (g) + O2 (g) ↔ 2 SO3 (g) ∆H = -192.3 kJ
19. If you add more oxygen gas, which way will equilibrium shift?
20. If you decrease pressure, which way will equilibrium shift?
21. If you add a catalyst, which way will equilibrium shift?
22. If you decrease the temperature, which way will equilibrium shift?
23. If you decrease the volume, which way will equilibrium shift?
24. List the common properties of acids and bases.
25. Which is stronger, Nitric Acid [H3O+] = 1.5 x 10-4 or Sulfuric Acid [H3O+] = 6.2 x 10-7
26. Which is a stronger acid, lemon juice (pH =2) or milk (pH = 6)?
27. What is a Brönsted-Lowry acid? What is a Brönsted-Lowry base?
28. Using the Brönsted-Lowry definitions of acids and bases, identify the acid, base, conjugate acid and conjugate base in the following reaction. H2SO4 + NH3 → HSO4- + NH4+
29. What are the reactants and products of a neutralization reaction?
30. Calculate the pOH of a solution with a pH of 4.5.
31. What is the [OH-] of a solution with a pH of 9.8?
32. Calculate the pH of a solution with a [H3O+] of 3.7 x 10-4
33. What is the [H3O+] of a solution whose pH is 2.35?
34. The following data were collected at the endpoint of a titration to find the molarity of HCl.
Volume of acid (HCl) used = 10.0 mL
Volume of base (NaOH) used = 25.0 mL
Molarity of base (NaOH) = 0.30 M
What is the molarity of the acid solution?
35. You are titrating HF with 4.20 M lithium hydroxide. The indicator in phenolphthalein. You have 25.5 mL of HF and you titrate in 58.7 mL of LiOH. What is the concentration of the HF solution?
36. 65 mL of 0.15 M barium hydroxide is added to 53 mL of 0.35 M hydrochloric acid (barium chloride and water are produced). What is the concentration of the barium chloride after the reaction?
a. Balanced equation:
b. Moles of barium chloride produced:
c. Molarity of barium chloride:
37. If I leave 500. mL of 0.75 M magnesium chloride solution uncovered on a windowsill and 120. mL of the solvent evaporates, what is the new concentration of the solution?
38. Will the following substances dissolve in water or oil: Calcium chloride, Methanol (CH3OH) and Copper (II) sulfate
39. Assuming a 525.0 mL, 0.420 M solution of Ascorbic Acid (C6H8O6) has a density of 1.3 g/mL, what is the percent by mass concentration?
40. What does a Keq > 1 mean? What about a Keq < 1?