A scientist adds a solution of AgNO3 (aq) dropwise to a solution conta.docx

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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 10â€“10 Ksp(AgBr) = 5.4 x 10â€“13 Ksp(AgI) = 8.5 x 10â€“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 .

Educación

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

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