For the dissociation of hydrogen cyanide in aqueous solution, i.e. #HC-=N(aq) + H_2O(l) rightleftharpoons H_3O^+ + ""^(-):C-=N#... which scenario will change the equilibrium constant?
#"a. adding more hydrocyanide;"#
#"b. raising the temperature;"#
#"c. adding more solvent;"#
#"d. adding another acid."#
Only (b) will (possibly) change the equilibrium constant.
Hydrocyanic (prussic) acid undergoes the acid-base reaction as follows:
As with any equilibrium reaction, we can write the acid-base dissociation expression,
Now I don't know the value of
I take it that this is a 1st year problem?