Chem. 12 Review Test 2
Pick two formulas that match each classification:
1.
2.
3.
4.
Acid
Covalent Nonacid
Salt
Base
a) Ba(NO3)2
b) CH3COO H
c) H2O
d) Al(OH)3
e) NaBr
f) C3H8
g) H3PO4
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)
Final burette reading (mL)
2.05
10.56
10.56
19.09
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 and
30.0 mL of 0.200 M KOH 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.
What concentration of acid or base remains when 200.0 mL of 0.200 M H2SO4 is
mixed with 200.0 mL 0.100 M KOH and 400 mL 0.100 M NaOH.