HCN dissociates into CN- and protons. A) What is the equilibrium constant at T=298.15 K? B)...

HCN dissociates into CN- and protons.

A) What is the equilibrium constant at T=298.15 K?

B) At what pH will the reaction move to the left if the solution contains 0.1 M HCN?

Solutions

Expert Solution

A) Since we know an equillibrium constant is related to the standard Gibbs free energy change for the reaction.

G = -RTlnK

finding G for HCN is equal to +124.7 KJ/mol

lnK = 124.7 / - 8.314 x 298.15

lnK = 124.7 / - 2478.8191

lnk = - 0.05030

K = e^(-0.05030)

= 0.951

B) HCN H⁺ + CN^-

At 0.1M HCN pH = 1 from pH table we get know that if H+ ions concentration increases then pH decreases here in this concerned can say reaction will get in forward direction. and if pH will be greater than 1 then reaction will move left in direction.

queen_honey_blossom answered 1 year ago

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