Consider the dissociation of hydrocyanic acid in aqueous solution HCN - CN + H* for which K, is 4.9 x 101°. (i) Find the pH of a solution initially 102 M in HCN, and the degree of dissociation of the HCN, a. (ii) To this solution is added more CN' until [CN'] = (0.1 M. What is the new pH of the solution? (ii) Without making a new numerical cakculation, explain qualitatively how the degree of dissociation would change if the solution is diluted.

Consider the dissociation of hydrocyanic acid in aqueous solution HCN - CN + H* for which K, is 4.9 x 101°. (i) Find the pH of a solution initially 102 M in HCN, and the degree of dissociation of the HCN, a. (ii) To this solution is added more CN' until [CN'] = (0.1 M. What is the new pH of the solution? (ii) Without making a new numerical cakculation, explain qualitatively how the degree of dissociation would change if the solution is diluted.

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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Consider the dissociation of hydrocyanic acid in aqueous solution
HCN - CN + H*
for which K, is 4.9 x 101°.
(i) Find the pH of a solution initially 102 M in HCN, and the degree of dissociation of the HCN, a.
(ii) To this solution is added more CN' until [CN'] = (0.1 M. What is the new pH of the solution?
(ii) Without making a new numerical cakculation, explain qualitatively how the degree of dissociation
would change if the solution is diluted.

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