Download 1 - AlvarezHChem

1.
2.
Calculate the molarity of each of these solutions.
A.
A 5.623g sample of NaHCO3 is dissolved in enough water to make a
250.0 mL of solution.
B.
A 184.6mg sample of K2Cr2O7 is dissolved in enough water to make
500.0mL of solution.
C.
A 0.1025g sample of copper metal is dissolved in 35mL of
concentrated HNO3 to form Cu+2 ions and then water is added to make
a total volume of 200.0mL. What is the molarity of Cu+2 in the final
solution?
Calculate the concentration of all the ions present in each of the following
solutions of strong electrolytes.
A.
B.
C.
0.15M calcium chloride
0.26M aluminum nitrate
0.25M potassium chromate
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3.
4.
Describe how you would prepare 2.00 liters of each of the following solutions.
A.
0.250M NaOH from solid NaOH
B.
0.250M NaOH from 1.00M NaOH stock solution
C.
0.100M K2CrO4 from solid K2CrO4
D.
0.100M K2CrO4 from 1.75M K2CrO4 stock solution
A solution is prepared by dissolving 10.8g ammonium sulfate in enough water
to make 100.0mL of stock solution. A 10.00mL sample of this stock solution
is added to 50.0mL of water. Calculate the concentration of ammonium ions
and sulfate ions in the final solution.
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5.
6.
When the following solutions are mixed together, what precipitate (if any)
will form? Write the equations for each in #6
A.
barium chloride and sodium sulfate
B.
lead (II) nitrate and potassium chloride
C.
silver nitrate and sodium phosphate
D.
sodium hydroxide and iron (III) nitrate
For question #5 above, write the formula equation, ionic equation and net
ionic equation for each combination.
A) F: ______________________________________________________________
I: ______________________________________________________________
NI: ____________________________________________________________
B) F: ______________________________________________________________
I: ______________________________________________________________
NI: ____________________________________________________________
C) F: ______________________________________________________________
I: ______________________________________________________________
NI: ____________________________________________________________
D) F: ______________________________________________________________
I: ______________________________________________________________
NI: ____________________________________________________________
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7.
Write the formula equation, ionic equation, and net ionic equation for the
reactions that occur between the following combinations:
A.
ammonium sulfate and barium nitrate
F: ______________________________________________________________
I: ______________________________________________________________
NI: ____________________________________________________________
B.
sodium phosphate and potassium nitrate
F: ______________________________________________________________
I: ______________________________________________________________
NI: ____________________________________________________________
C.
copper (II) chloride and sodium hydroxide
F: ______________________________________________________________
I: ______________________________________________________________
NI: ____________________________________________________________
8.
What mass of Na2CrO4 is required to precipitate all of the silver ions from
75.0mL of a 0.100M solution of AgNO3? (Hint: this involves stoichiometry
and the molarity formula)
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Write the chemical formula based on the name and then assign oxidation numbers
to all of the elements in the compound. Remember to show your work.
(NOTE: arsenate = AsO4-3; iodate = IO3-1; bromate = BrO3-1)
1)
potassium sulfate
8)
tin (II) nitrate
2)
sodium perchlorate
9)
chromium (III) iodate
3)
carbonic acid
10)
barium phosphate
4)
cesium arsenate
11)
iron (II) nitrite
5)
zinc dichromate
12)
lead (II) permanganate
6)
chloric acid
13)
aluminum carbonate
7)
gallium chromate
14)
cobalt (II) bromate
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