Concentration of ammonia in a solution


by sveioen
Tags: ammonia, concentration, solution
sveioen
sveioen is offline
#1
Nov5-07, 12:08 AM
P: 14
Hello all,

I had chemistry a long time ago, but now I am very rusty at it so I am hoping you can get me started with this problem I have;

A particular solution of ammonia (Kb = 1.8 x 10-5) has a pH of 8.3.
What is the concentration of ammonia in this solution?

Is it the concentration of NH3 I have to find? I know I can find [OH-] since I know the pH, but what does the final equation look like? Something like [tex]Kb=[OH-][NH4+]/[NH3][/tex]?

Thank you for any help!
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Antineutron
Antineutron is offline
#2
Nov5-07, 12:28 AM
P: 76
NH4 and OH- is going to have same amount of equilibrium concentration gained from the NH3. So If you know the pH, then how do you find the pOH, and what is the concentration of OH-? Multiply both sides by NH3 and divide bothsides by Kb. What happens?
sveioen
sveioen is offline
#3
Nov5-07, 12:37 AM
P: 14
Ok, so pOH = 14 - pH = 14 - 8,3 = 5,7. Concentration of OH- and NH4 is therefore [tex]1,995 \times 10^{-6}[/tex]? And then [tex] [NH3] = \frac{[OH^-][NH4^+]}{K_b}[/tex]?

Antineutron
Antineutron is offline
#4
Nov5-07, 12:48 AM
P: 76

Concentration of ammonia in a solution


So plug the values and see what you get, I hope this answer agree with the true answer, does it?? If not tell me.
sveioen
sveioen is offline
#5
Nov5-07, 12:54 AM
P: 14
I got [tex]2,21 \times 10^{-7}[/tex], which seems reasonable I guess. Maybe a bit low?!
Antineutron
Antineutron is offline
#6
Nov5-07, 12:59 AM
P: 76
You don't have the answer? It should be reasonable right? because its the equilibrum concentration right?
sveioen
sveioen is offline
#7
Nov5-07, 01:09 AM
P: 14
Nope dont have answer (yet) :(, but it seems kinda right.. Probably is equilibrum concentration..
lightarrow
lightarrow is offline
#8
Nov8-07, 06:08 AM
P: 1,504
Quote Quote by sveioen View Post
I got [tex]2,21 \times 10^{-7}[/tex], which seems reasonable I guess. Maybe a bit low?!
I got [tex]2,21 \times 10^{-6}[/tex] instead.


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