Solid AgNo3 is added slowly to solution of 0.001M Cl,Br,and I
a)
at what concentration of Ag will AgI precipitating?
at what concentration of Ag will AgCl precipitating?
at what concentration of Ag will AgBr precipitating?
b)
calculate the percent % of I ppt before reaching of AgBr?
calculate the percent % of Br ppt before reaching of AgCl?
Ksp AgI = (Ag^+)(I^-)
You know Ksp and I^-, solve for Ag^+.
Same for AgBr and AgCl.
b part.
What is Ag^+ when AgBr first ppts. You calculated that above. Plug Ag+ from the AgBr when it first ppt into Ksp for AgI to find the I^- concn when AgBr starts. Then %I left at that point is [(I^-)/0.001]*100 = ? That's what's left so % pptd is 100%- ?%. There isn't much left and essentially all has been pptd. AgBr is done the same way.
Post your work if you need help understanding any of this.
thanksssss
I see what you said we used the Ag from AgBr to find the [I] by using the Ksp for AgI
To determine at what concentration of Ag (silver) each compound will start precipitating, we need to compare the solubility product constant (Ksp) values of each compound with the concentration of Ag in the solution.
a)
First, let's find the solubility product constants for each compound:
AgI: Ksp = [Ag+][I-]
AgCl: Ksp = [Ag+][Cl-]
AgBr: Ksp = [Ag+][Br-]
For AgI:
The solubility product constant (Ksp) for AgI is 8.3 x 10^-17 at 25°C.
At the point of AgI precipitation, the concentration of Ag will be equal to the solubility product constant for AgI.
So, [Ag] = 8.3 x 10^-17 M.
For AgCl:
The solubility product constant (Ksp) for AgCl is 1.8 x 10^-10 at 25°C.
At the point of AgCl precipitation, the concentration of Ag will be equal to the solubility product constant for AgCl.
So, [Ag] = 1.8 x 10^-10 M.
For AgBr:
The solubility product constant (Ksp) for AgBr is 5.0 x 10^-13 at 25°C.
At the point of AgBr precipitation, the concentration of Ag will be equal to the solubility product constant for AgBr.
So, [Ag] = 5.0 x 10^-13 M.
b)
To calculate the percent (%) of I precipitate before reaching the point of AgBr precipitation, we need to compare the concentration of AgI with the concentration of AgBr when AgBr starts precipitating.
We have the concentration of Ag for AgI precipitation ([Ag] = 8.3 x 10^-17 M) and AgBr precipitation ([Ag] = 5.0 x 10^-13 M).
The percent (%) of I precipitate before reaching the point of AgBr precipitation can be calculated as follows:
% of I ppt = ([Ag]_AgI / [Ag]_AgBr) x 100
Substituting the values:
% of I ppt = (8.3 x 10^-17 / 5.0 x 10^-13) x 100
Performing the calculation, we get the percentage of I precipitate.
To calculate the percent (%) of Br precipitate before reaching the point of AgCl precipitation, we follow the same approach as above.
We have the concentration of Ag for AgBr precipitation ([Ag] = 5.0 x 10^-13 M) and AgCl precipitation ([Ag] = 1.8 x 10^-10 M).
The percent (%) of Br precipitate before reaching the point of AgCl precipitation can be calculated as follows:
% of Br ppt = ([Ag]_AgBr / [Ag]_AgCl) x 100
Substituting the values:
% of Br ppt = (5.0 x 10^-13 / 1.8 x 10^-10) x 100
Performing the calculation, we get the percentage of Br precipitate.