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13 Dec 2019

Aqueous solutions of NH3 and HCN react to produce NH4CN according to the following equilibrium reaction.

NH3(aq) +HCN(aq) <---> NH4+(aq) +CN-(aq)

Given the following equilibrium constants, which statement best describes the reaction once equilibrium is established? (Kw=1.01x10^-14) and why?

NH4+ Ka = 5.6x10^-10
HCN Ka=4.0x10^-10

A. The reaction is running in forward direction.
B. The reaction is running in reverse direction
C. The reaction is neither product nor reactant favored

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Nelly StrackeLv2

17 Dec 2019

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Related questions

Consider a salt of a weak base and a weak acid such as ammonium cyanide. Both the NH₄⁺ and CN⁻ ions interact with water in an aqueous solution, but the net reaction can be considered as a proton transfer from NH₄⁺ to CN⁻.

NH₄⁺ (aq) + CN⁻ (aq) ⇌ NH₃ (aq) + HCN (aq)

Show that the equilibrium constant for this reaction, K act, is 1. K net = Ka Kb Kw where Ka is the ionization constant for the weak acid NH₄⁺ and Kb is the constant for the weak base CN⁻
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