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1. Question: If you dissolved 72.1 grams of NaBr (molecular mass 102.89 g/mol) in water to prepare 500 ml of solution, what is the molarity of this solution?
2. Question: If a sample of gas with a volume of 20 ml at a pressure of 6 ATM is moved to an area with a pressure of 2 ATM, what is the new volume of the gas?
3. Question: You prepare a solution by dissolving CaCl₂ in water to make a 3.0 M solution. What is the osmolarity of this solution?
4. Question: At a fixed temperature and pressure, a 6.0 mole sample of an ideal gas occupies 134.4 L. After using up some of this gas, I have 104.0 L of gas left in my sample. How many moles of gas do I now have in my sample?
5. Question: When 0.3 grams of potassium iodide is dissolved in 60 ml of water in a beaker, the solute is:
6. Question: You have 2.4 L of a 5.6 M LiCl solution. How many L of a 3.2 M LiCl solution could you produce by diluting this solution?
7. Question: Balance the following chemical equation: C₇H₁₆ + O₂ → CO₂ + H₂O. Which of the below represents this properly balanced reaction?
8. Question: Consider the compound with the chemical formula (NH₄)₂SO₄. What is the molecular mass of this compound?
9. Question: In the acid-base reaction: KOH + HBr → H₂O + KBr. What is the base in the chemical reaction?
10. Question: You dissolve a sample of LiCl in water. The molarity of this solution is 0.3 M. What is the osmolarity of this solution?
11. Question: You have 0.4 moles of C₃H₈ that you combust (balanced chemical reaction is: C₃H₈ + 3 O₂ → 3 CO₂ + 4 H₂O), how many moles of CO₂ will you generate?
12. Question: You added 2 grams of HCl to 80 ml of water. What would you expect to occur?
13. Question: Predict the products of this neutralization reaction. Select all that apply. HCl + RbOH → ?
14. Question: When the following reaction goes in the forward direction, what is the base?
    NH₄⁺ (aq) + H₂O (l) → NH₃ (aq) + H₃O⁺ (aq)
15. Question: Glucose, an important biomolecule, has a molar mass of 180.16 g/mol. If I had 4 moles of glucose, how would I express this amount in grams?
16. Question: You are looking at the results of a series of tests to determine if a series of solutions, A-E, would be considered acidic. Select ALL that you think are acidic based on the results below:
17. Question: The conjugate base of HCN would be:
18. Question: A 1.4 mole sample of gas at 57 K occupies 0.5 L in a 13.1 ATM atmosphere. Which of these variables represents the pressure?
19. Question: According to the Kinetic Molecular Theory of gases, what do we assume about collisions between gas molecules in an ideal gas?
20. Question: Calculate the volume, in L, of a 2.4 mole sample of oxygen gas at a pressure of 14.6 ATM at 16°C. Show all work below.
21. Question: If you decreased the temperature of a sample of gas, what would you expect to happen to the volume of the gas at a fixed pressure?
22. Question:6 moles of NaHCO₃ decompose following the balanced reaction below. How many moles of H₂O will you form? Show all work.
23. Question: For the following, consider a balloon filled with gas. Assuming ideal gas behavior, predict the effect:
24. Question: A solution is prepared by dissolving 100 g of CaF₂ in water to a total volume of 670 mL. What is the mass/volume % concentration of this solution?
25. Question: In a container, a 7 mole sample of gas occupies 300 L at a pressure of 1.5 ATM. What must be the temperature of the gas in this container?
26. Question: Balance the chemical equation: HCl + O₂ → Cl₂ + H₂O.
27. Question: You are trying to determine which solutions are buffers by adding a few drops of base to each solution and measuring the change in pH. Based on the data below, which solution would you classify as buffers? Select all that apply.
28. Question: You are preparing a buffered solution. So far, your solution contains H₃PO₄. What ions would you add to this solution to prepare your buffer system?
29. Question: I have 32.0 grams of N₂. How many moles of N₂ do I have?
30. Question: What would be the products of the neutralization equation below? Select all that apply. HCl + Ca(OH)₂ → ?