12:23 LTE question 16 MasteringChemistry An aqueous solution that 1.90 M in AgNO

Question

12:23 LTE question 16 MasteringChemistry An aqueous solution that 1.90 M in AgNO is slowly added from a buret to an aqueous solution that is 1.00x10-2 M in Cl and 0.240 M in I Part A Which ion, Cl orI, is the first to precipitate? Cl Submit Request Answer Part B When the second ion begins to precipitate, what is the remaining concentration of the first ion? Express your answer using two significant figures Submit Request Answer Part C Is the separation of Cl and I feasible by fractional this solution? yes

Explanation / Answer

(A)

The iodide ion (I-) will precipitate first because Ksp value for AgI is smaller.

(B)

At this point we have:

Ksp = [Ag+]*[Cl-] = 1.77*10-10

Putting values:

[Ag+]*0.01 = 1.77*10-10

So,

[Ag+] = 1.77*10-8

Now we have:

Ksp = [Ag+]*[l-] = 8.52*10-17

Putting values:

[1.77*10-8]*[I-] = 8.52*10-17

Solving we get:

[I-] = 4.81*10-9 M

Hope this helps !

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