Question

A 115.0 −mL sample of a solution that is 2.6×10−3 M in AgNO3 is mixed with a 220.0 −mL sample of a solution that is 0.14 M in NaCN. A complex ion forms. After the solution reaches equilibrium, what concentration of Ag+(aq) remains?

Answer 1

A 115.0 mL of AgNO₃ solution with 2.6x10^-3M is mixed with a 220.0 mL of NaCN solution 0.14M

Volume total: 115.0 mL + 220.0 mL = 335.0 mL = 0.335 L

Determine the mole for each reactive:

Determine the mole for each ions:

Concentration:

Concentration:

The formation constant for the complex ions is very large, so we can assume nearly all of the Ag⁺ are in the complex ion form. Kf=1.0x10²¹ (from a chemistry book)

Equation			+
Initial (M)
Change
Equilibrium (M)