In: Chemistry
Cyanide is used in several industrial applications, such as mining gold and electroplating silver. A danger of working with cyanide solutions is the potential hazard of releasing highly toxic hydrogen cyanide gas. What conditions are necessary to ensure that less than 1% of the cyanide in a particular solution is chemically present as HCN rather than CN-? (HCN pKa= 9.2)
(A) pH > 11.2
(B) pH > 10.2
(C) pH > 9.2
(D) pH > 8.2
(E) pH > 7.2
(F) pH < 11.2
(G) pH < 10.2
(H) pH < 9.2
(I) pH < 8.2
(J) pH < 7.2
-Please explain, Thank you.
From the question it is clear that [HCN]/[CN-] must be less than 1%
Since, less than 1% of the cyanide should be present as HCN rather than CN-. This implies [HCN] < 1% Ionization reaction of HCN is: HCN ---> H+ + CN- pKa = 9.2 Ka = [H+][CN-] / [HCN] For pKa = pH , CN- and HCN will be present in equal amounts i.e [CN-] = [HCN] For pKa < pH , [CN-] > [HCN] For pKa > pH , [CN-] < [HCN]
Hence when pH > 9.2 then more conc of CN- would be there than HCN.
Now , we want to calculate the conditions when [HCN]< 1%
So, [HCN]/[CN-] < 1% .........(1)
since , Ka = [H+][CN-] / [HCN] , so [HCN]/[CN-] = [H+]/Ka Putting this in equation (1) [H+]/Ka = [HCN]/[CN-] < 1% [H+]/Ka < 1/100 Taking log both sides : log [H+] - log(Ka) < log(10-2) Multiplying -1 both sides: -log [H+] - (-log(Ka)) > 2 (inequality sign changes on multiplication by a negative number) pH - pKa > 2 pH > 2 + pKa pH > 2 + 9.2 pH > 11.2
For pH>11.2, less than 1% of HCN is present in the solution.