A solution contains 0.020 mole each of I¯, Br¯, and Cl¯, When the solution is mixed with 200. mL of 0.29 M AgNO3, what mass of AgCI(s) precipitates out, and what is [Ag*]? Assume no volume change. AgI: Ksp = 1.5 x 10¬16 AgBr: Kp = 5.0 × 10¬13 AgCl: К,р — 1.6 х 10-10 Mass = g (Ag*]=| M
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![A solution contains 0.020 mole each of I, Br¯, and Cl¯. When the solution is mixed with 200. mL of 0.29 M AgNO3, what mass of AgCl(s) precipitates out, and what is [Ag*]?
Assume no volume change.
AgI:
Ksp = 1.5 x 10-16
AgBr: Ksp
- 5.0 × 10-1
AgCl: Ksp
1.6 x 10-10
Mass
[Ag*] =[
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3216a391-9091-4165-86c6-f10847a236cf%2F273ba84a-30ca-4f3b-a766-18112db28117%2F4e358ha_processed.png&w=3840&q=75)
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