HCl(aq) + H2O(l) ⇄ H3O+(aq) + Cl−(aq) In 1.0M HCl(aq), HCl is nearly 100 percent dissociated, as represented by the equation above. Which of the following best helps to explain why, in 0.01M HCN(aq), less than 1 percent of HCN is dissociated?
a) The CN− ion is not very soluble in water, and a solid precipitate would form if more of the HCN dissociated.
b) Compared to the HCl(aq) solution, the concentration of the HCN(aq) solution is much too dilute to achieve 100 percent dissociation.
c) The equilibrium constant for the dissociation of HCN(aq) is much smaller than that for the dissociation of HCl(aq).
d) HCN(aq) reacts with water to form a basic solution, and the high concentration of OH−(aq) interferes with the dissociation process.