Review of Chemistry 11
In order to be successful in Chemistry 12, there are several key concepts from Chemistry 11 that you must master. We will spend two periods in class reviewing these concepts. I challenge you to get 86 % or higher on this test. I believe that everyone in this class can get this mark. You need to convince yourself that you can, then, do then work and you will. This worksheet contains everything that will be tested. I can give you a practice test if you want one. If you need help, that’s what I am here for- see me.
HCl C
3
H
8
SO
2
NH
4
Cl KOH H
2
SO
4
H
2
O AgNO
3
PbSO
4
H
3
PO
4
Ca(OH)
2
Al(OH)
3
P
2
O
5
Ba(OH)
2
CH
3
COOH NaCl
1. Classify each of the above chemical formulas by placing them to the right of the correct heading.
Salts
Bases
Acids
Nonacids
2. Calculate the molar mass of FeSO
4
•
5H
2
O and Co
3
(PO
4
)
2
•
6H
2
O.
3. 0.300 moles of NaCl is dissolved in 250.0 mL of water, calculate the molarity.
4. 500. g of FeSO
4
6H
2
O is dissolved in 600. mL of water, calculate the molarity.
5. How many grams of NaCl are required to prepare 100.0 mL of a 0.200 M solution?

6. 20. g of MgCl
2
are dissolved in 250.0 mL of water, calculate the concentration of each ion.
7. How many liters of 0.300 M NaCl contains10.0 g of NaCl?
8. For each double replacement reaction write the formula equation, the complete ionic equation and the net ionic equation. a) H
3
PO
4(aq)
+ Sr(OH)
2(aq)
→
Na
3
PO
4(aq)
→ b) Ca(NO
3
)
2(aq)
+ c) Zn(s) + HCl
(aq)
→

9. In three runs of a titration 22.8, 22.1 and 22.2 mL of 0.200 M Ba(OH)
2
were required to neutralize 10.0 mL of HCl, calculate the acid concentration.
10. In three runs of a titration 12.1, 12.8, 12.8 mL of 0.200 M HCl were required to neutralize 10.0 mL of Ca(OH)
2
, calculate the base concentration.
11. 35.0 mL of 1.00 M H
2
SO
4
reacts with 175 mL 0.250 M NaOH, calculate the concentration of the excess acid.
12. 350.0 mL of 0.200 M HCl reacts with 175 mL 0.125 M Ca(OH)
2
, calculate the concentration of the excess acid.
13. 25.0 g of sodium reacts with water, how many grams of hydrogen are produced? How many grams of sodium hydroxide are produced?

14. 25.0 g of calcium reacts with water, how many grams of calcium hydroxide are produced?
15. How many millilitres of 0.200M NaOH is required to neutralize 25.0 mL of 0.100 M
H
2
SO
4
?
16. How many millilitres of 0.200 M H
2
SO
4
is required to neutralize 25.0 mL of 0.100 M
NaOH ?
17. If the [F
-
] = 0.600 M in an AlF
3 solution, calculate [Al
3+
] and the number of grams required to make 1.00 L of the solution.
18. If the [Na
+
] = 0.250 M in a Na
3
P solution, calculate [P
3-
] and the number of grams required to make 1.50 L of the solution.

19. A beaker has a mass of 25.36 g. A solution that contains 2.00 L of a solution of BaCl
2
has a mass of 163.59 g. The solution is evaporated to dryness and it then has a mass of 28.59 g. Calculate the molarity of the solution.
20. 200.0 mL of 0.100 M Na
3
PO
4
is mixed with 100.0 mL of 0.200 M Na
2
SO
4.
Calculate all ion concentrations. There is no reaction in the situation as the solutions are just diluting each other and the [Na + ] increases. First write out two dissociation equations. Use dilution factors to lower each concentration. Add the two [Na
+
] concentrations together at the end to get the total.
21. In a titration 0.175 M H
2
C
2
O
4
was added to a 25.00 mL sample of NaOH. The following data was collected. Calculate the molarity of the base.
Final volume of H
2
C
2
O
4
(mL)
Initial volume of H
2
C
2
O
4
(mL)
Trial #1
23.00
4.85
Trail # 2
39.05
23.00
Trial #3
20.95
5.00

22. 2HCl + Ba(OH)
2
→ BaCl
2
+ 2 H
2
O
When 3.16 g samples of Ba(OH)
2
were titrated to the endpoint with HCl solution.
37.80mL, 35.49mL, 35.51 mL of HCL was required. Calculate the HCl concentration.