× Didn't find what you were looking for? Ask a question
Top Posters
Since Sunday
a
5
k
5
c
5
B
5
l
5
C
4
s
4
a
4
t
4
i
4
r
4
r
4
Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
New Topic  
nf_7138 nf_7138
wrote...
solved
13 years ago
If 200.mL of a 0.00500M solution of AgNO3 were added to 400.mL of a 0.0100M solution of Na2CrO4, would Ag2CrO4 precipitate? The Ksp of Ag2CrO4 is 1.1 x 10^-12
Read 1947 times
1 Reply

Related Topics

Replies
wrote...
#1
Staff Member
13 years ago
Balanced Reaction:

2 Ag+ (aq) + CrO42- (aq) Rightwards Arrow Ag2CrO4 (s)

Ksp = [Ag+]2 times [CrO4-]

If [CrO4-] = x, then [Ag+] = 2x (from the balanced equation)
then Ksp = 2x2 * x = 4x3 (substitute in for Ksp equation)

Solve for 'x'.

Max Concentration of CrO42- that is saturated in solution is: ...
Max Concentration of Ag2+ that is saturated in solution is: 2*(whatever number you get for 'x') = ...

Compare to actual concentration in solution:

Ag2+: 200 mL * ( 0.00500M / 1000 mL ) = ...
CrO42-: 400 mL * ( 0.0100M / 1000mL) = ...

If the actual amount of both ions in solution is greater than the maximum amount that will be saturated, then all the excess will precipitate out.
- Master of Science in Biology
- Bachelor of Science
New Topic      
Quick Reply
Explore
Post your homework questions and get free online help from our incredible volunteers
  1231 People Browsing
 123 Signed Up Today
Start New Topic Take the Tour CoursesNew Study Tools Topics Trending Browse by Textbook
Related Images
  
 151
  
 661
  
 134
Your Opinion
Which 'study break' activity do you find most distracting?
Votes: 741
Previous poll results: Who's your favorite biologist?