Chem. 12 Review Test 2
Pick two formulas that match
each classification:
1.
Acid a) Ba(NO3)2 e) NaBr
2.
Covalent
Nonacid b) CH3COO H f) C3H8
3.
Salt c)
H2O g) H3PO4
4.
Base d)
Al(OH)3 h) Ca(OH)2
5. A student wants to determine the molarity of 100.0 mL of NaCl
solution. She weighs another empty beaker and determines the mass to be 56.23 g.
She transfers all of the solution to this beaker, weighs it, and finds the mass
to be 159.99 g. She proceeds to evaporate off the water until it is dry and
measures the mass of the beaker and residue to be 58.69 g. What is the molarity
of the solution?
6. How many grams of AlCl3 are required to prepare 250.0
mL of 0.200 M solution?
7. How many litres of 0.350 M MgCl2 are needed to provide
250.0 g of MgCl2?
8. 50.6 g of AlCl3 is dissolved in 250.0 mL H2O,
calculate [Al3+] and [Cl-].
9. 600.0 mL of 0.200 M H2SO4 reacts with 600.0
mL of 0.200 M NaOH. Calculate concentration of the excess acid in the new
solution.
10. In three runs of a titration 0.200 M NaOH was used to neutralize a
25.0 mL sample of H2CO3. Calculate the molarity of the
acid.
|
0.200 M NaOH in the burette |
|
|
|
|
Initial burette reading
(mL) |
2.05 |
10.56 |
19.09 |
|
Final burette reading (mL) |
10.56 |
19.09 |
27.80 |
|
|
|
|
|
11. How many grams of .0200 M H2C2O4
are required to neutralize 250.0 mL of .0250 M KOH?
12. Complete the reaction equations.
i) Formula Equation/Chemical Equation
Sr(OH)2 (aq) +
ZnSO4 (aq)
ii) Total Ionic Equation
iii) Net Ionic Equation
13. Write the complete ionic equation for the reaction of Mg (s)
and HCl (aq).
14. What volume of 0.100 M H2SO4 is needed to
neutralize 25.0 mL 0.250 M NaOH solution?
15. Calculate all ion concentrations after 200.0 mL of 0.200 M CaCl2
is mixed with 200.0 mL of 0.300 M AlCl3.
16. An impure sample of CaC2O4 weighing 0.633
g is dissolved in water and the reacted with 12.20 mL of 0.120 M KMnO4.
Calculate the percent by mass of CaC2O4 in the original
sample.
2MnO4- +
5C2O42- +
16H+ ® 2Mn2+ + 10CO2 + 8H2O