A scientist adds a solution of AgNO3 (aq) dropwise to a solution conta.docx
A scientist adds a solution of AgNO3 (aq) dropwise to a solution containing a mixture of 0.01 M NaCl (aq), 0.01 M NaBr (aq), and 0.01 M NaI (aq). Given the data below, which solid would be the first to precipitate out of solution? Ksp(AgCl) = 1.8 x 10–10 Ksp(AgBr) = 5.4 x 10–13 Ksp(AgI) = 8.5 x 10–17 Solution given 0.01 M NaBr ---> 0.01 M Br- 0.01 M NaCl ----> 0.01 M Cl- 0.01 M NaI ----> 0.01 M I- now due to common ion effect , the contributions are of these respective ions are taken now AgCl (s) ---> Ag+ + Cl- Ksp = [Ag+] [Cl-] 1.8 x 10-10 = [Ag+] x 0.01 [Ag+] = 1.8 x 10-8 2) AgBr (s) ---> Ag+ + Br- Ksp =[Ag+][Br-] 5.4 x 10-13 = [Ag+] x 0.01 [Ag+] = 5.4 x 10-11 3) AgI (s) ---> Ag+ + I- Ksp = [Ag+] [I-] 8.5 x 10-17 = [Ag+] x 0.01 [Ag+] = 8.5 x 10-15 now AgNO3 is very much soluble in water and for the remaining AgI is the first to precipitate out of the solution since it only need 8.5 x 10-15 M Ag+ , the lowest so the answer is AgI .
A scientist adds a solution of AgNO3 (aq) dropwise to a solution conta.docx
A scientist adds a solution of AgNO3 (aq) dropwise to a solution containing a mixture of 0.01 M NaCl (aq), 0.01 M NaBr (aq), and 0.01 M NaI (aq). Given the data below, which solid would be the first to precipitate out of solution? Ksp(AgCl) = 1.8 x 10–10 Ksp(AgBr) = 5.4 x 10–13 Ksp(AgI) = 8.5 x 10–17 Solution given 0.01 M NaBr ---> 0.01 M Br- 0.01 M NaCl ----> 0.01 M Cl- 0.01 M NaI ----> 0.01 M I- now due to common ion effect , the contributions are of these respective ions are taken now AgCl (s) ---> Ag+ + Cl- Ksp = [Ag+] [Cl-] 1.8 x 10-10 = [Ag+] x 0.01 [Ag+] = 1.8 x 10-8 2) AgBr (s) ---> Ag+ + Br- Ksp =[Ag+][Br-] 5.4 x 10-13 = [Ag+] x 0.01 [Ag+] = 5.4 x 10-11 3) AgI (s) ---> Ag+ + I- Ksp = [Ag+] [I-] 8.5 x 10-17 = [Ag+] x 0.01 [Ag+] = 8.5 x 10-15 now AgNO3 is very much soluble in water and for the remaining AgI is the first to precipitate out of the solution since it only need 8.5 x 10-15 M Ag+ , the lowest so the answer is AgI .
![A scientist adds a solution of AgNO3 (aq) dropwise to a solution containing a mixture of 0.01 M
NaCl (aq), 0.01 M NaBr (aq), and 0.01 M NaI (aq). Given the data below, which solid would be
the first to precipitate out of solution?
Ksp(AgCl) = 1.8 x 10–10
Ksp(AgBr) = 5.4 x 10–13
Ksp(AgI) = 8.5 x 10–17
NaNO3 (s)
Solution
given 0.01 M NaBr ---> 0.01 M Br-
0.01 M NaCl ----> 0.01 M Cl-
0.01 M NaI ----> 0.01 M I-
now
due to common ion effect , the contributions are of these respective ions are taken
now
AgCl (s) ---> Ag+ + Cl-
Ksp = [Ag+] [Cl-]
1.8 x 10-10 = [Ag+] x 0.01
[Ag+] = 1.8 x 10-8
2)](https://image.slidesharecdn.com/ascientistaddsasolutionofagno3aqdropwisetoasolutionconta-230203005609-fe4329db/75/a-scientist-adds-a-solution-of-agno3-aq-dropwise-to-a-solution-contadocx-1-2048.jpg?cb=1675387550)
![AgBr (s) ---> Ag+ + Br-
Ksp =[Ag+][Br-]
5.4 x 10-13 = [Ag+] x 0.01
[Ag+] = 5.4 x 10-11
3) AgI (s) ---> Ag+ + I-
Ksp = [Ag+] [I-]
8.5 x 10-17 = [Ag+] x 0.01
[Ag+] = 8.5 x 10-15
now
AgNO3 is very much soluble in water
and for the remaining
AgI is the first to precipitate out of the solution since it only need 8.5 x 10-15 M Ag+ , the
lowest
so
the answer is AgI](https://image.slidesharecdn.com/ascientistaddsasolutionofagno3aqdropwisetoasolutionconta-230203005609-fe4329db/75/a-scientist-adds-a-solution-of-agno3-aq-dropwise-to-a-solution-contadocx-2-2048.jpg?cb=1675387550)
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A scientist adds a solution of AgNO3 (aq) dropwise to a solution conta.docx
- 1. A scientist adds a solution of AgNO3 (aq) dropwise to a solution containing a mixture of 0.01 M NaCl (aq), 0.01 M NaBr (aq), and 0.01 M NaI (aq). Given the data below, which solid would be the first to precipitate out of solution? Ksp(AgCl) = 1.8 x 10–10 Ksp(AgBr) = 5.4 x 10–13 Ksp(AgI) = 8.5 x 10–17 NaNO3 (s) Solution given 0.01 M NaBr ---> 0.01 M Br- 0.01 M NaCl ----> 0.01 M Cl- 0.01 M NaI ----> 0.01 M I- now due to common ion effect , the contributions are of these respective ions are taken now AgCl (s) ---> Ag+ + Cl- Ksp = [Ag+] [Cl-] 1.8 x 10-10 = [Ag+] x 0.01 [Ag+] = 1.8 x 10-8 2)
- 2. AgBr (s) ---> Ag+ + Br- Ksp =[Ag+][Br-] 5.4 x 10-13 = [Ag+] x 0.01 [Ag+] = 5.4 x 10-11 3) AgI (s) ---> Ag+ + I- Ksp = [Ag+] [I-] 8.5 x 10-17 = [Ag+] x 0.01 [Ag+] = 8.5 x 10-15 now AgNO3 is very much soluble in water and for the remaining AgI is the first to precipitate out of the solution since it only need 8.5 x 10-15 M Ag+ , the lowest so the answer is AgI