THE SOLUBILITY PRODUCT CONSTANT
(Ksp) OF SILVER ACETATE
In a saturated solution, the ions in solution are in
equilibrium with the solid. The rate at
which ions are leaving the solid crystal is equal to the rate at which they are
returning to the crystal:
AgCH3CHOO(s) ø Ag+1(aq) + CH3COO-1(aq)
The concentrations of the ionic species, Ag+1
and CH3COO-1, when no net change in concentration is
taking place, determine the equilibrium solubility. The equilibrium constant expression for this reaction is:
Ksp = [Ag+1] [CH3COO-1]
If pure silver acetate is dissolved, the acetate ion
concentration is the same as the silver ion concentration*. Thus, the solubility product constant can be
calculated after experimentally determining the equilibrium concentration of
either ion.
In this experiment, you will determine the equilibrium
concentration of the silver ion in a saturated solution of silver acetate at
room temperature. The reaction between
Cu(s) and Ag+1(aq) is the same one which we studied in SCH 3A.
Procedure:
(Day 1)
1.
Carefully
measure, in a 100 mL graduated cylinder, 100 mL of a saturated silver acetate
solution. Pour the solution into a
clean, dry 250 mL beaker.
2.
Obtain
about 30 cm of 16 gauge copper wire.
Clean the surface of the wire with some emery cloth or file and wind the
wire into a loose coil around a test tube.
3.
Find
the mass of the copper coil to the nearest 0.01 g and place it into the beaker
containing the saturated solution of silver acetate. Allow the system to stand overnight so all the silver ions will
have an opportunity to react.
(Day 2)
4.
Shake
the silver crystals free from the copper wire into the beaker. Wash any adhering crystals into the beaker
with a stream of distilled water from a water bottle.. Finally, wash the wire in a stream of water
from the tap. When the wire is dry,
find its mass.
5.
Decant
the solution off the silver crystals and rinse them with distilled water. Place the silver into a container designated
by your teacher so it can be used again.
*
small differences due to hydrolysis of acetate are neglected here
Calculations and Results:
1.
Calculate
the number of moles of Cu(s) which reacted with the silver ions.
2.
Recall
the relationship between Cu(s) and Ag+1(aq). How many moles of silver ions were present
in the 100 mL sample? What is the
concentration of the silver ions in moles per liter?
3.
What
is the concentrations of the acetate ions present in the solution, expressed in
mol/L?
4.
Calculate
the value of Ksp for silver acetate at room temperature.
5.
If
100 mL of 0.02 M silver nitrate and 100 mL of 0.02 M sodium acetate were mixed,
would a precipitate of silver acetate be expected to form? Show all of your work.
6.
Suppose
that some solid sodium acetate was added to the saturated solution of silver
acetate. After the sodium acetate is
dissolved, what will be the effect of the increased concentration of the
acetate ion on the equilibrium: (Le Chatelier)
AgCH3CHOO(s) ø Ag+1(aq) + CH3COO-1(aq)
7.
Calculate
the concentration of the silver ions if the acetate ion concentration in the
solution of question 6 is 1.0 M.