1. Chemistry Jeopardy
SINGLE JEOPARDY

2. Solutions
Electrolytes
Equilibrium
Molarity
Acid-Base
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3. A solution must consist of a solute and ?
Question A-1
A solution must consist of a solute and ?

4. Answer
Solvent.

5. Question A-2
If a substance was insoluble, could you make a solution with it? EXPLAIN.

6. No, it could not be a solute if it can not dissolve.
Answer
No, it could not be a solute if it can not dissolve.

7. Ex.) Pure substance, ionic compound, etc…
Question A-3
Properly classify a solution in terms of the classification of matter?
Ex.) Pure substance, ionic compound, etc…

8. Would be a homogenous mixture.
Answer
Would be a homogenous mixture.

9. What is the mathematical expression for concentration?
Question A-4
What is the mathematical expression for concentration?

10. Answer
M=moles of solute/total volume of solution. (M=moles/Liters is acceptible)

11. Question A-5
What is the difference between a stock solution and a diluted solution?

12. Answer
A stock solution is more concentrated, has more solute, less solvent than a diluted solution.

13. What kind of electrolyte is NaCl, strong, weak or non?
Question B-1
What kind of electrolyte is NaCl, strong, weak or non?

14. Answer
Strong

15. What would NaCl(s) look like dissociated?
Question B-2
What would NaCl(s) look like dissociated?

16. Answer
Na+ and Cl-

17. What are the 7 molecules that full disociate?
Question B-3
What are the 7 molecules that full disociate?

18. HCl HBr HI HNO3 H2SO4 HClO4 HClO3
Answer
HCl
HBr HI
HNO3
H2SO4
HClO4
HClO3

19. Question B-4
What kind of electrolyte would have ionized and non ionized particles in solution?

20. Answer
Weak

21. Question B-5
Arrange the following from most conductive to least conductive: HCl, H2SO4, Li3N, C2H6, HC2H3O2

22. Answer
Li3N
H2SO4
HCl
HC2H3O2
C2H6

23. What kind of arrow is used in an equilibrium chemical equation?
Question C-1
What kind of arrow is used in an equilibrium chemical equation?

24. Answer
Double sided 

25. CaCO3(s) CaO(s)+ CO2(g)
Question C-2
What would the equilibrium constant expression be for the following reaction?
CaCO3(s) CaO(s)+ CO2(g)

26. Answer
k= [CO2]

27. Use the following equation to answer the question.
Question C-3
Use the following equation to answer the question.
N2(g) + 3H2(g)  2NH3(g)
If hydrogen was added, what way would the equilibrium shift?

28. Answer
Shift right or forward

29. Use the following equation to answer the question.
Question C-4
Use the following equation to answer the question.
N2(g) + 3H2(g)  2NH3(g)
If the volume of the container decreased, which way would the equilibrium shift?

30. Answer
Shift right or forward

31. Use the following equation to answer the question.
Question C-5
Use the following equation to answer the question.
N2(g) + 3H2(g)  2NH3(g)
If argon gas was added to the system in a rigid container, what way would the equilibrium shift?

32. Answer
It wouldn’t. The addition of Ar gas wouldn’t affect the concentrations of the species in the reaciton.

33. What is the molarity of a solution that has 2 moles in 2.0L?
Question D-1
What is the molarity of a solution that has 2 moles in 2.0L?

34. Answer
1.0M

35. Question D-2
What would the molarity be of a solution that was created with 55.5g of calcium chloride in 500.0mL of water

36. Answer
1.0M

37. How many moles of HCl would exist in 600.0mL of a 3.0M solution?
Question D-3
How many moles of HCl would exist in 600.0mL of a 3.0M solution?

38. Answer
1.8 moles

39. Question D-4
How many liters would a sample containing 0.75 moles and having a concentration of 2.0M be?

40. Answer
0.375L

41. Question D-5
Calculate how many mL of an 16.0M stock solution you would need to create 200.0mL of a 0.6M dilution?

42. Answer
7.5mL

43. What element does every acid have to have?
Question E-1
What element does every acid have to have?

44. Answer
Hydrogen

45. What is the conjugate base of nitric acid?
Question E-2
What is the conjugate base of nitric acid?

46. Answer
NO3-

47. In the following reaction is water acting as an acid or base?
Question E-3
In the following reaction is water acting as an acid or base?
NH3 + H2O  NH4+ + OH-

48. Answer
Acid

49. Question E-4
Why is it that every bronsted lowry base can not be considered an arrhenius base?

50. Answer
A substance that can accept an H+ does not always have to ionize to produce OH- ions.

51. Question E-5
One sample containing 200.0mL of a 0.6M HCl solution was mixed with another sample containing 250.0mL of a 0.45M solution. After the acid-base reaction was complete what would the [H+] and [OH-] be?.

52. Answer
[H+]=0.0167
[OH-]=0