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 .

equilibrium constant Kc = 8.52 × 10⁻⁴

Explanation:

You  need The equations for the dissolution of AgI(s) and the stability constant of the  complex [Ag(CN)₂]⁻(aq)

The equations for the dissolution of AgI(s) is:

AgI(s)   ⇔   Ag⁺(aq)  +  I⁻(aq)               Ksp  =   [Ag⁺(aq) I⁻(aq)]

The stability constant of the  complex [Ag(CN)₂]⁻(aq) is:

Ag⁺(aq)  +     2CN⁻(aq)    ⇔  [Ag(CN)₂]⁻(aq)        Kfb2 =

Adding the equations for the dissolution of AgI(s) and the stability constant of the  complex [Ag(CN)₂]⁻(aq) we get the required reaction. so the equilibrium   constant for the reaction is the product of the individual equilibrium constants:

AgI(s)     +     2CN⁻(aq)  ⇔   [Ag(CN)₂]⁻(aq)   +  I⁻(aq)

Kc = Ksp  × Kfb2  =    [Ag⁺(aq) I⁻(aq)]   ×    =  

Kc =  8.52 × 10⁻¹⁷  ×  1  × 10²¹  = 8.52 × 10⁻⁴

hope this

explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)

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