Determine the molar solubility ( ) of zn(cn)2 in a solution with a ph=1.33 . ignore activities. the for zn(cn)2 is 3.0×10−16 . the for hcn is 6.2×10−10 .

Explanation:

We have to determine the molar solubility of in the given solution.

So, let molar solubility is x.

                       0           x        2x

Also, HCN upon dissociation gives

So, concentration of hydrogen ion equals the concentration of cynaide ion. Therefore, calculate the concentration of hydrogen ion using the pH value as follows.

                           pH = -log

                          1.33 = -log

                     antilog (-1.33) =

                          =

Let molar solubility of hydrogen and cyanide ions is "a".

                          0        a        a

Also,       =

                           = x            

                           =       ( x + a = a because a >> x)          

                                 x =

                             =

                             =

Thus, we can conclude that molar solubility of in the given solution is .

the answer is a and have a great day