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     C3H8        SO2    NH4Cl    KOH    H2SO4    H2O    AgNO3    PbSO4     H3PO4    Ca(OH)2     Al(OH)3    P2O5    Ba(OH)2   CH3COOH

 

1. Classify the above as ionic or covalent by making two lists. Describe the difference between an ionic and covalent compound.

 

 

 

 

 

 

 

2. Classify the above as acids, bases, salts and molecular (covalent compounds) by making four lists.

 

 

 

 

3. Describe how you can identify each of the four categories by the formula of the compound.

 

 

 

 

4. Describe how each of the four categories would react with litmus and conduct electricity when aqueous.

 

 

 

 

 

5. For each compound that conducts electricity, write a dissociation equation to show how it ionizes in water.

 

 

 

 

6. Calculate the molar mass of FeSO4 • 5H2O and Co3(PO4)2 • 6H2O.

 

 

7. 0.300 moles of NaCl is dissolved in 250.0 mL of water, calculate the molarity.

 

 

 

 

 

 

 

8. 500. g of FeSO4 6H2O is dissolved in 600. mL of water, calculate the molarity.

 

 

 

 

 

 

 

 

9. How many grams of NaCl are required to prepare 100.0 mL of a 0.200 M solution?

 

 

 

 

 

 

 

 

10. 20. g of MgCl2 are dissolved in 250.0 mL of water, calculate the concentration of each ion.

 

 

 

 

 

 

 

 

11. How many liters of 0.300 M NaCl contains10.0 g of NaCl?

 

 

 

 

 

 

 

 

 

 

12.       For each double replacement reaction write the formula equation, the complete ionic equation and the net ionic equation.

 

a)         H2SO4(aq)         +          NaOH(aq)          →

 

 

 

 

b)         H3PO4(aq)          +          Sr(OH)2(aq)       →

 

 

 

 

c)         Ca(NO3)2(aq)     +          Na3PO4(aq)        →

 

 

 

 

d)         Zn(s)                +          HCl(aq)             →

 

 

 

 

13.       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.

 

 

 

 

 

 

 

 

 

 

 

 

14.       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.

 

 

 

 

 

 

15.       35.0 mL of 1.00 M H2SO4 reacts with 175 mL 0.250 M NaOH, calculate the concentration of the excess acid.

 

 

 

 

16.       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.

 

 

 

 

 

 

 

 

 

 

17.       25.0 g of sodium reacts with water, how many grams of hydrogen are produced? How many grams of sodium hydroxide are produced?

 

 

 

 

 

 

 

 

18.       25.0 g of calcium reacts with water, how many grams of hydrogen are produced? How many grams of calcium hydroxide are produced?

 

 

 

 

 

 

 

 

19.       How many millilitres of 0.200M NaOH is required to neutralize 25.0 mL of  0.100 M H2SO4 ?

 

 

 

 

20.       How many millilitres of 0.200 M H2SO4 is required to neutralize 25.0 mL of 0.100 M NaOH ?

21.       If the [F-] = 0.600 M in an AlF3 solution, calculate [Al3+] and the number of grams required to make 1.00 L of the solution.

 

 

 

 

 

 

 

22.       If the [Na+] = 0.250 M in a Na3P solution, calculate [P3-] and the number of grams required to make 1.50 L of the solution.

 

 

 

 

 

 

 

 

 

 

23.       A beaker has a mass of 25.36 g. A solution that contains 2.00 L of a solution of BaCl2 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.

 

 

 

 

 

 

 

 

 

 

24.       A beaker of mass = 55.66g contains 1.00 L of a solution of AlF3 and is evaporated to dryness mass = 62.31 g. Calculate the molarity of the solution.

 

 

 

 

 

 

 

 

 

 

25.       In a titration 0.175 M H2C2O4 was added to a 25.00 mL sample of NaOH. The following data was collected. Calculate the molarity of the base.

 

 

Trial #1

Trail # 2

Trial #3

Final volume of H2C2O4 (mL)

23.00

39.05

20.95

Initial volume of H2C2O4 (mL)

4.85

23.00

5.00

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

26.       2HCl     +    Ba(OH)2   ----------->   BaCl2    +    2 H2O

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.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

27.       A 0.960 g sample of impure Na2CO3 is dissolved in water and then completely reacted with 0.200 M HCl requiring 6.53 mL. Calculate the percentage by mass of Na2CO3 in the sample.

 

            Na2CO3            +          2HCl   ®        CO2            +          2NaCl              +            H2O