Question

Calculate the value of the equilibrium constant, K c , for the reaction AgI ( s ) + 2 CN − ( aq ) − ⇀ ↽ − [ Ag ( CN ) 2 ] − ( aq ) + I − ( aq ) K c = ? The solubility product constant, K sp , for AgI is 8.52 × 10 − 17 , and the formation constant, K f ( β 2 ), for [ Ag ( CN ) 2 ] − is 1.0 × 10 21 .

Answer 1

The equilibrium constant, Kc, for the reaction AgI (s) + 2 CN- (aq) <=> [Ag(CN)2]- (aq) + I- (aq) can be calculated using the solubility product constant (Ksp) for AgI and the formation constant (Kf) for [Ag(CN)2]-.

Step-by-step explanation:

The equilibrium constant, Kc, for the reaction AgI (s) + 2 CN- (aq) <=> [Ag(CN)2]- (aq) + I- (aq) can be calculated using the solubility product constant (Ksp) for AgI and the formation constant (Kf) for [Ag(CN)2]-.

1. First, we write the expression for Ksp for AgI, which is equal to the product of the concentrations of Ag+ and I-. Ksp = [Ag+][I-].
2. Next, we write the expression for Kf for [Ag(CN)2]-, which is equal to the product of the concentrations of Ag+ and CN- squared. Kf = [Ag+][CN-]2.
3. Finally, we multiply Ksp and Kf to calculate Kc, the equilibrium constant for the reaction. Kc = Ksp * Kf.

Using the given values for Ksp (8.52 x 10-17) and Kf (1.0 x 1021), we can substitute these values into the equation to calculate Kc.