2. Acid/Base
pH and
pOH
Solubility
Molarity
Neutral-
ization
100
100
100
100
100
200
200
200
200
200
300
300
300
300
300
400
400
400
400
400
500
500
500
500
500

3. This is a H+ acceptor. A. Acid B. Base C. Neutral
?1 $100
This is a H+ acceptor. A. Acid B. Base C. Neutral B

4. This turns red litmus paper blue. A. Acid B. Base C. Neutral
?1 $200
This turns red litmus paper blue. A. Acid B. Base C. Neutral B

5. Ca(OH)2 A. Acid B. Base C. Neutral
?1 $300
Ca(OH)2 A. Acid B. Base C. Neutral B

6. ?1 $400
pH of 1.5 (Use strong or weak in your response) A. Strong acid B. Weak acid C. Strong base D. Weak base E. Neutral A

7. A H+ donator. A. Acid B. Base C. Neutral
?1 $500
A H+ donator. A. Acid B. Base C. Neutral A

8. ?2 $100
pH of HCl A. 1 B. 3 C. 11 D. 14 B

9. ?2 $200
pOH of M NaOH A. 1 B. 5 C. 9 D. 14 B

10. ?2 $300
pH of 0.01 M Ca(OH)2 A. 1 B. 2 C. 12 D. 14 C

11. ?2 $400
pOH of M HCl A. 1 B. 5 C. 9 D. 14 C

12. H+ concentration of water A. 1 x 10-7 B. 1 x 10-14 C. 7 D. 14
?2 $500
H+ concentration of water A. 1 x 10-7 B. 1 x C. 7 D. 14 A

13. ?3 $100
Cooling does this to solubility. A. Increases B. Decreases C. No Change B

14. ?3 $200
To dilute a solution you should add more of this. A. Solute B. Solvent C. Solution B

15. This is not changed in a dilution.
?3 $300
This is not changed in a dilution.
Original
Diluted
A. mL of water
50mL
100mL
B. Mass of
solution
100g
150g
C. Moles of
solute
2.0 C

16. ?3 $400
A solution where no more solute molecules can dissolve. (it is just right!) A. Unsaturated B. Saturated C. Supersaturated B

17. ?3 $500
Using this solubility curve: this is the number of grams of NH4Cl that can dissolve in 100 g of water at 70°. A. 60 g B. 74 g C. 90 g D. cannot tell from this graph A

18. ?4 $100
This is the concentration of a solution with 1.0 moles in 500mL of solution. A M B. 0.5 M C. 1 M D. 2 M E. 500 M D

19. ?4 $200
This is the effect on Molarity when more solvent is added to the solution. A. Increases B. Decreases C. No change
B – larger denominator when the solvent (L) increases

20. ?4 $300
What is the concentration of 2.0 L of solution that has 50.0g of NH3? A. 1.5 M B. 25 M C. 425 M D M A

21. ?4 $400
This is the number of grams of NH3 needed to make 3.00L of a M solution. A g B g C g D. 102 g C

22. ?4 $500
This is the volume of 18M Hydrochloric acid needed to make 0.100L of 2M solution. A L B. 0.9 L C. 180 L D. 360 L A

23. ?5 $100
This is the process we use in the lab to reach neutralization. A. Molarity B. Dilution C. Titration D. Agitation C

24. ?5 $200
This is the number of moles of HCl needed to neutralize 6 moles of NaOH. A. 6 moles B. 12 moles C. 18 moles A

25. ?5 $300
This is the balanced equation when HCl and NaOH react. A. HCl + NaOH  H2O + NaCl B. HCl + H2O  Cl- + H3O+ C. HCl + H2O  H2O + NaCl A

26. ?5 $400
What is the concentration of sulfuric acid (H2SO4) when 25mL are used to neutralize 30mL of 0.20M sodium hydroxide (NaOH). A M B M C M D M A

27. ?5 $500
You have two un-labled HCl solutions: 0.15M and 1.5M. You use 0.020L of acid to neutralize 0.5M NaOH. What statement is true. A. If you used 0.06L of base the acid is 1.5M. B. If you use 0.006L of base the acid is 1.5M. C. If you used 0.06L of base the acid is 0.15 M. D. An equal amount of base will neutralize 0.15 M and 1.5 M solutions A