If 450 mL of 1 times 10^-7 M AgNO3 is mixed with 450 mL of 1 times 10 M Nal, wha

Question

If 450 mL of 1 times 10^-7 M AgNO3 is mixed with 450 mL of 1 times 10 M Nal, what will occur? For Agl, Ksp = 8.3 times 10^-17 A) Silver(I) iodide will precipitate. B) No precipitate will form. C) Sodium nitrate will precipitate. D) Silver(I) nitrate will precipitate. E) Sodium iodide will precipitate. Sodium chloride is added slowly to a solution that is 0.010 Min Cu^+, Ag^+, .and Au^+. The, K_ip values for the chloride salts are 1.9 times 10^-7, 1.6 times 10^-10, and 2.0 times 10^-13, respectively. Which compound will precipitate first? A) CuCl (s) B) AgCl (s) C) AuCl(s) D) All will precipitate at the same time E) It cannot be determined.

Explanation / Answer

Q10.

First, identify ions in solution

Ag+ NO3- Na+ and I-

Note that Silver halides are not soluble, so there could be AgI(S) precipitation

recall that

AgI(S) <-> Ag+ + I-

Ksp = [Ag+][I-]

so

if Q >> KSp, expect superstauration of AgI, so precipitates forms

[Ag+] = M1*V1/(V1+V2) = 450 * (10^-7)/(450+450) = 5*10^-8 M

[I-] = M2*V2/(V1+V2) = 450 *(10^-8) / (450+450) = 5*10^-9 M

now

Q = [Ag+][I-] = (5*10^-8)(5*10^-9) = 2.5*10^-16

since

Q > Ksp

expect AgI precipitation

AgI, silver ioidide will precipitate (E)

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