1-Consider the reaction when aqueous solutions of magnesium sulfate and manganese (II) nitrate are combined. The net ionic equation for this reaction is: 2-Consider the reaction when aqueous solutions of lead nitrate and aluminum sulfate are combined. The net ionic equation for this reaction is: 3-Consider the reaction when aqueous solutions of ammonium phosphate and sodium iodide are combined. The net ionic equation for this reaction is: 4-Consider the reaction when aqueous solutions of magnesium bromide and potassium phosphate are combined. The net ionic equation for this reaction is: 5-Consider the reaction when aqueous solutions of ammonium sulfide and magnesium sulfate are combined. The net ionic equation for this reaction is: 6-Consider the reaction when aqueous solutions of potassium nitrate and barium sulfide are combined. The net ionic equation for this reaction is: 7-Consider the reaction when aqueous solutions of sodium sulfide and potassium nitrate are combined. The net ionic equation for this reaction is: 8-Consider the reaction when aqueous solutions of ammonium phosphate and potassium nitrate are combined. The net ionic equation for this reaction is: 9-Consider the reaction when aqueous solutions of iron(III) nitrate and copper(II) sulfate are combined. The net ionic equation for this reaction is: 10-How many mL of 0.406 M HI are needed to dissolve 5.97 g of CaCO3? 2HI(aq) + CaCO3(s)  CaI2(aq) + H2O(l) + CO2(g)  mL 11-A 0.5488 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated asAgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 1.1541 g.  What is the mass percentage of chlorine in the original compound?   % 12-A student determines the aluminum content of a solution by first precipitating it as aluminum hydroxide, and then decomposing the hydroxide to aluminum oxide by heating. How many grams of aluminum oxide should the student obtain if her solution contains 51.0 mL of 0.583 M aluminumnitrate?  g 13-Write a net ionic equation to show that hydrobromic acid, HBr, behaves as an acid in water. 14-Write a net ionic equation to show why solid potassium hydroxide, KOH (s), forms a basic solution when it dissolves in water. 15-The substance ethylamine is a weak nitrogenous base like ammonia. Write a net ionic equation to show how ethylamine, C2H5NH2, behaves as a base in water. 16-Write a net ionic equation for the reaction that occurs when aqueous solutions of sodium hydroxide and hydrobromic acid are combined.  17-Write a net ionic equation for the reaction that occurs when aqueous solutions of potassium hydroxide andhypochlorous acid are combined. 18-Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and acetic acid are combined 19-Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrobromic acid and ammonia are combined ...

1. 1-Consider the reaction when aqueous solutions of magnesium
sulfate and manganese (II) nitrate are combined. The net ionic
equation for this reaction is:
2-Consider the reaction when aqueous solutions of lead
nitrate and aluminum sulfate are combined. The net ionic
equation for this reaction is:
3-Consider the reaction when aqueous solutions of ammonium
phosphate and sodium iodide are combined. The net ionic
equation for this reaction is:
4-Consider the reaction when aqueous solutions of magnesium
bromide and potassium phosphate are combined. The net ionic
equation for this reaction is:
5-Consider the reaction when aqueous solutions of ammonium
sulfide and magnesium sulfate are combined. The net ionic
equation for this reaction is:
6-Consider the reaction when aqueous solutions of potassium
nitrate and barium sulfide are combined. The net ionic equation
for this reaction is:
7-Consider the reaction when aqueous solutions of sodium
sulfide and potassium nitrate are combined. The net ionic
equation for this reaction is:
8-Consider the reaction when aqueous solutions of ammonium
phosphate and potassium nitrate are combined. The net ionic
equation for this reaction is:
9-Consider the reaction when aqueous solutions of iron(III)
nitrate and copper(II) sulfate are combined. The net ionic
equation for this reaction is:

2. 10-How many mL of 0.406 M HI are needed to dissolve 5.97 g
of CaCO3?
2HI(aq) + CaCO3(s) CaI2(aq) + H2O(l) + CO2(g)
mL
11-A 0.5488 g sample of a pure soluble chloride compound is
dissolved in water, and all of the chloride ion is precipitated
asAgCl by the addition of an excess of silver nitrate. The mass
of the resulting AgCl is found to be 1.1541 g.
What is the mass percentage of chlorine in the original
compound?
%
12-A student determines the aluminum content of a solution by
first precipitating it as aluminum hydroxide, and then
decomposing the hydroxide to aluminum oxide by heating. How
many grams of aluminum oxide should the student obtain if her
solution contains 51.0 mL of 0.583 M aluminumnitrate?
g
13-Write a net ionic equation to show that hydrobromic
acid, HBr, behaves as an acid in water.

3. 14-Write a net ionic equation to show why solid potassium
hydroxide, KOH (s), forms a basic solution when it dissolves in
water.
15-The substance ethylamine is a weak nitrogenous base like
ammonia.
Write a net ionic equation to show how ethylamine,
C2H5NH2, behaves as a base in water.
16-Write a net ionic equation for the reaction that occurs when
aqueous solutions of sodium hydroxide and hydrobromic
acid are combined.
17-Write a net ionic equation for the reaction that occurs when
aqueous solutions of potassium hydroxide andhypochlorous
acid are combined.
18-Write a net ionic equation for the reaction that occurs when
aqueous solutions of ammonia and acetic acid are combined
19-Write a net ionic equation for the reaction that occurs when
aqueous solutions of hydrobromic acid and ammonia are
combined
20-Write a net ionic equation for the reaction that occurs
when excess hydriodic acid (aq) and lead(II) carbonate are
combined.
21-Write a net ionic equation for the reaction that occurs
when ammonium sulfide and excess hydriodic acid (aq) are
combined.
22-What volume of a 0.138 M perchloric acid solution is
required to neutralize 24.9 mL of a 0.196 M calcium

4. hydroxidesolution?
mL perchloric acid
23-What volume of a 0.174 M potassium hydroxide solution is
required to neutralize 28.3 mL of a 0.310 M hydrobromic
acid solution?
mL potassium hydroxide
24-An aqueous solution of calcium hydroxide is standardized by
titration with a 0.196 M solution of perchloric acid.
If 24.9 mL of base are required to neutralize 12.6 mL of the
acid, what is the molarity of the calcium hydroxide solution?
M calcium hydroxide
25-An aqueous solution of potassium hydroxide is standardized
by titration with a 0.174 M solution of hydrobromic acid.
If 28.3 mL of base are required to neutralize 24.0 mL of the
acid, what is the molarity of the potassium hydroxidesolution?

5. M potassium hydroxide
26-A 14.0 g sample of an aqueous solution of perchloric
acid contains an unknown amount of the acid.
If 29.2 mL of 0.946 M sodium hydroxide are required to
neutralize the perchloric acid, what is the percent by weight
ofperchloric acid in the mixture?
% by weight
27-A 9.00 g sample of an aqueous solution of hydrobromic
acid contains an unknown amount of the acid.
If 24.9 mL of 1.17 M sodium hydroxide are required to
neutralize the hydrobromic acid, what is the percent by weight
of hydrobromic acid in the mixture?
% by weight
28-Potassium hydrogen phthalate is a solid, monoprotic acid
frequently used in the laboratory to standardize strong base
solutions. It has the unwieldy formula of KHC8H4O4. This is
often written in shorthand notation as KHP.
How many grams of KHP are needed to exactly
neutralize 25.6 mL of a 0.537 M potassium hydroxide solution ?
grams KHC8H4O4

6. 29-Potassium hydrogen phthalate is a solid, monoprotic acid
frequently used in the laboratory to standardize strong base
solutions. It has the unwieldy formula of KHC8H4O4. This is
often written in shorthand notation as KHP.
What volume of a 0.437 M potassium hydroxide solution is
needed to exactly neutralize 2.76 grams of KHP ?
ANSWER:
mL potassium hydroxide
30-
The oxidation number of an element is the "charge" the element
would have if all of its bonds were completely ionic; that is, if
the electron pairs of each bond were transferred to the more
electronegative atom.
For monatomic ions the oxidation number is simply the charge
of the ion. For covalently bonded elements the oxidation
number is a bookkeeping device and does not mean that the
element carries an actual charge.
Determine the oxidation state for each of the elements below.
The oxidation state of
...
nitrogen
...
in

7. ...
nitrite ion
NO2-
...
is
...
.
The oxidation state of
xenon
in
xenon gas
Xe
is
.
The oxidation state of
bromine
in
bromate ion
BrO3-
is
.

8. 31-
Use the rules (in order) to assign oxidation numbers to each of
the elements in the compounds below.
boric acid
H
B
O
H3BO3
hypochlorite ion
Cl
O
ClO-
periodic acid
H
I

9. O
HIO4
32-
N2 + 4Fe(OH)2+ 4H2O4Fe(OH)3 + N2H4
In the above redox reaction, use oxidation numbers to identify
the element oxidized, the element reduced, the oxidizing agent
and the reducing agent.
name of the element oxidized:
name of the element reduced:
formula of the oxidizing agent:
formula of the reducing agent:
33-
Mn(OH)2 + HPbO2-Pb + MnO2+ H2O+ OH-

10. In the above redox reaction, use oxidation numbers to identify
the element oxidized, the element reduced, the oxidizing agent
and the reducing agent.
name of the element oxidized:
name of the element reduced:
formula of the oxidizing agent:
formula of the reducing agent:
34-A student is asked to standardize a solution of potassium
hydroxide. He weighs out 1.02 g potassium hydrogen phthalate
(KHC8H4O4, treat this as a monoprotic acid).
It requires 36.9 mL of potassium hydroxide to reach the
endpoint.
A. What is the molarity of the potassium hydroxide solution?
M

11. This potassium hydroxide solution is then used to titrate an
unknown solution of hydrochloric acid.
B. If 23.4 mL of the potassium hydroxide solution is required to
neutralize 27.6 mL of hydrochloric acid, what is the molarity of
the hydrochloric acid solution?
M
35-A student is asked to standardize a solution of sodium
hydroxide. He weighs out 1.02 g potassium hydrogen phthalate
(KHC8H4O4, treat this as a monoprotic acid).
It requires 31.9 mL of sodium hydroxide to reach the endpoint.
A. What is the molarity of the sodium hydroxide solution?
M
This sodium hydroxide solution is then used to titrate an
unknown solution of nitric acid.
B. If 18.0 mL of the sodium hydroxide solution is required to
neutralize 15.0 mL of nitric acid, what is the molarity of
the nitric acid solution?
M
36-Consider the reaction when aqueous solutions of copper(II)
bromide and silver acetate are combined. The net ionic equation
for this reaction is:
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