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J-7
(4.0)
15.
(Exp E)
a)
Write the balanced net ionic equation for the reaction between cadmium nitrate, Cd(NO3)2, and
sodium oxalate, Na2C2O
4
.
b)
In each of the following test tubes, 5.0 mL of 0.10 M Cd(NO3)2 and 5.0 mL of
0.10 M Na2C2O
4
were combined and allowed to stand for 10 minutes in order to reach
equilibrium. The following additions were made to these test tubes:
test tube #1 -
2.0 mL of distilled water
test tube #2 -
2.0 mL of 1.0 M HCl, hydrochloric acid
test tube #3 -
2.0 mL of 1.0 M HNO3, nitric acid
The solutions were mixed thoroughly, allowed to stand to reach equilibrium again, then the
observations were recorded.
Using LeChatelier's Principle, explain how the reaction in part a) of this question would be
affected by these additions. Give the expected visual observations and include all appropriate
interactive equilibria in your answers.
(4.0)
16.
(Exp F) In performing this experiment, the equilibrium for the following reaction was studied:
I
2(aq)
+ I
-
(aq)
I3
-
(aq)
,
A student determined that the total concentration of ( I2 and I3
-
) in the aqueous layer was
0.0120 M. Calculate:
a)
the [I3
-
] in the aqueous layer, given that [I
2(aq)
] was 2.10 x 10
-4
M
b)
the [I
-
] in the aqueous layer, given that the original KI3 solution was prepared from
0.100 M KI.
c)
the equilibrium constant, K
eq
, using your answers from parts a) and b)
