Use values of Ksp for AgI and Kf for Ag(CN)2− to calculate the molar solubility of AgI in pure water, calculate the equilibrium constant for the reaction Agl(s)+2CN−(aq)⥫⥬==Ag(CN)−2(aq)+I−( aq), determine the molar solubility of AgI in a 0.100 M NaCN solution.

a)

b) Keq = 8.3x10⁴

c)  

Explanation:

a) To find the molar solubility of AgI in water we need to use the solubility product constant (Ksp) of the following reaction:

AgI(s)  ⇄  Ag⁺(aq) + I⁻(aq)

Since [Ag⁺] = [I⁻]:

Hence, the molar solubility of AgI in water is 9.11x10⁻⁹ mol/L.

b) The equilibrium constant of AgI in CN, first we need to evaluate the reactions involved:

AgI(s)  ⇄  Ag⁺(aq) + I⁻(aq)   (1)

  (2)

Ag⁺(aq) + 2CN⁻(aq)  ⇄  Ag(CN)₂⁻(aq)   (3)

  (4)

The net equation is given by the sum of the reactions (1) and (3):

AgI(s) + 2CN⁻(aq)  ⇄  Ag(CN)₂⁻(aq) + I⁻(aq)    (5)

Hence, the equilibrium constant of the reaction (5) is:

  (6)

From equation (2):

  (7)

By entering equations (7) and (4) into equation (6) we have:

Therefore, the equilibrium constant for the reaction (5) is 8.3x10⁴.  

c) From reaction (5):

AgI(s) + 2CN⁻(aq)  ⇄  Ag(CN)₂⁻(aq) + I⁻(aq)    

             0.1 - 2x                x                  x

Solving the above equation for x:

Hence, the molar solubility of AgI in a NaCN solution is 0.05 M.

I hope it helps you!

answer: the rate of diffusion increases with increase in temperature.

increase in temperature, increases the molecular/particles speed (kinetic energy. diffusion means movement of particles through the material.

generally, the heavier the particle the more it interacts with the environment and more the temperature matters. so higher temperature results in higher diffusion.