This preview shows pages 1–2. Sign up to view the full content.
Work Sheet 8+
CH302 Spring 2008
1.
A solution is made with NaI and NaCl such that it is 0.01 M in both I

and Cl

.
To 1 L of
this solution 0.01 moles Ag(NO
3
) are added (you can ignore any volume change).
The
NaI, NaCl, and Ag(NO
3
) are completely soluble (as is NaNO
3
but you already knew that).
The K
SP
for AgI is 8.3 x 10
17
and for AgCl is 1.8 x10
10
.
After the solution has reached equilibrium what are the concentrations of the following?
Will anything precipitate?
Initial concentration of [Ag
+
] is 0.01 M,
[I

] = 0.01 M,
[Cl

] = 0.01 M
Q
sp
= [Ag
+
][I

] = (.01)(.01) = 10
4
AgI could precipitate
Q
sp
= [Ag
+
][Cl

] = (.01)(.01) = 10
4
AgCl could precipate
However AgI is much less soluble than AgCl.
Assume the AgI precipitates completely to
equilibrium
Then you have a saturated solution of AgI
Concentration of Ag
+
will be
K
sp
= [Ag
+
][I

]
[Ag
+
] = sqrt(K
sp
) = sqrt(8.3 x 10
17
) = 9.11 x 10
9
Given this concentration will the AgCl precipitate?
Q
This preview has intentionally blurred sections. Sign up to view the full version.
View Full Document
This is the end of the preview. Sign up
to
access the rest of the document.
This homework help was uploaded on 04/12/2008 for the course CH 302 taught by Professor Holcombe during the Spring '07 term at University of Texas at Austin.
 Spring '07
 Holcombe
 Chemistry, Mole

Click to edit the document details