0.214 mol agno3 and 3.58 mol nh3 were added to enough water to give 1.00 l of solution at 25 °c. calculate the equilibrium concentration of free silver ion , [ag+], in this solution. the formation constant for ag(nh3)2+ (kf) = 1.50 x 10^7 at 25 °c.

Equilibrium concentration of free silver ion is 3.21×10^6 mol

Explanation: Since we have enough water in the reaction, we have aqueous NH3 reacting with AgNO3 (aq)

Equation of reaction:

AgNO3(aq) + 2NH3(aq) <> Ag(NH3)2+ at 25°C

Formation of complexes is also a thermal dynamic phenomenon. For the equilibrium,

Ag+ + 2NH3 <> Ag(NH3)2+

AgNO3(aq) + 2NH3(aq) <>Ag+ + 2NH3(aq)

•From the question, we have 0.214 mol of AgNO3 reacting with 3.58mol NH3 to produce a solution containing Ag(NH3)2+

•We can relate the number of moles to say that since we have 2 moles of NH3 reacting to form 2 moles of NH3 as product,

•Therefore 3.58mol of NH3 produces 3.58 mol of NH3 as well

AgNO3+ 2NH3 <> Ag+ + 2NH3

0.214mol 3.58mol 3.58mol

We can calculate the equilibrium concentration of free Ag+

Kf= [Ag+] [NH3]^2 / [AgNO3] [NH3]^2

Since we have [NH3]^2 as numerator and denominator we can easily cancel out both, leaving

Kf= [Ag+] / [AgNO3]

cross multiply

[Ag+] = Kf × [AgNO3]

Kf is given as 1.50× 10^7 at 25°C

Substitute into equation we have

[Ag+]= 1.50×10^7 × 0.214mol

[Ag+]= 3.21×10^6mol

Equilibrium concentration of free silver ion is 3.21×10^6 mol

the ratio of the conjugate base to the acid required to attain the desired ph.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.