What is the pH of 0.050 M Ba(CN)2 solution? please show work. Thank you.

What is the pH of 0.050 M Ba(CN)2 solution?

please show work. Thank you.

Expert Solution

Ba(CN)₂ is composed of a weak acid HCN and strong base Ba(OH)₂

The strong base remains dissociated while the weak acid tends to associate.

Thus, the following reaction takes place in a solution of Ba(CN)₂ :

CN^- + H₂O <----> HCN + OH^-

Initial 0.1 0 0

Equl. 0.1-x x x

For the above reaction, equilibrium constant, K = ( [HCN][OH-] )/[CN-] = x²/(0.1-x)

For HCN, Ka = 4.9*10^-10

Thus, K = Kw/Ka = 10^-14/(4.9*10^-10) = 2.04*10^-5

Thus, x²/(0.1-x) = 2.04*10^-5

Solving for the +ve value of x, we get :

x = 1.43*10^-3

Thus, pOH = -log x = 2.84

Thus, pH = 14-pOH = 11.16

queen_honey_blossom answered 2 hours ago

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