Part A A 130.0-mL sample of a solution that is 3.0 x 10-3 M in AgNO, is mixed with a 230.0-mL sample of a solution that is 0.14 M in NaCN. For Ag(CN)2, Ki = 1.0 × 1021. After the solution reaches equilibrium, what concentration of Ag*(aq) remains? Express your answer using two significant figures. ? [Ag*) = M Submit Request Answer
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A 130.0-mLmL sample of a solution that is 3.0×10−33.0×10−3 MM in AgNO3AgNO3 is mixed with a 230.0-mLmL sample of a solution that is 0.14 MM in NaCNNaCN. For Ag(CN)2−,Ag(CN)2−, Kf=1.0×1021Kf=1.0×1021. After the solution reaches equilibrium, what concentration of Ag+(aq)Ag+(aq) remains?
![Part A
A 130.0-mL sample of a solution that is 3.0 x 10 ³ M in AgNO3 is mixed with a 230.0-mL sample of a solution that is 0.14 M in NaCN. For
Ag(CN)2, K; = 1.0 × 102". After the solution reaches equilibrium, what concentration of Ag" (aq) remains?
Express your answer using two significant figures.
[Ag*] =
M
%D
Submit
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