The K sp value for Cu ( OH ) 2 and the overall formation constant for Cu ( NH 3 ) 4 2+ is given. The questions based on the stated data are to be answered. Concept introduction: The equilibrium constant for a given reaction is calculated by the formula, Equilibrium constant = K sp ⋅ K f At equilibrium, the equilibrium constant expression is expressed by the formula, K = Concentration of products Concentration of reactants
The K sp value for Cu ( OH ) 2 and the overall formation constant for Cu ( NH 3 ) 4 2+ is given. The questions based on the stated data are to be answered. Concept introduction: The equilibrium constant for a given reaction is calculated by the formula, Equilibrium constant = K sp ⋅ K f At equilibrium, the equilibrium constant expression is expressed by the formula, K = Concentration of products Concentration of reactants
Solution Summary: The author explains that the equilibrium constant for a given reaction is calculated by the formula, K_spcdot
Interpretation: The
Ksp value for
Cu(OH)2 and the overall formation constant for
Cu(NH3)42+ is given. The questions based on the stated data are to be answered.
Concept introduction: The equilibrium constant for a given reaction is calculated by the formula,
Equilibriumconstant=Ksp⋅Kf
At equilibrium, the equilibrium constant expression is expressed by the formula,
K=ConcentrationofproductsConcentrationofreactants
(b)
Interpretation Introduction
Interpretation: The
Ksp value for
Cu(OH)2 and the overall formation constant for
Cu(NH3)42+ is given. The questions based on the stated data are to be answered.
Concept introduction: The equilibrium constant for a given reaction is calculated by the formula,
Equilibriumconstant=Ksp⋅Kf
At equilibrium, the equilibrium constant expression is expressed by the formula,
The standard reduction potential for the reaction [Co(H2 O)6]3+(aq) + e− ⟶ [Co(H2 O)6]2+(aq) is about 1.8 V. The reduction potential for the reaction [Co(NH3)6]3+(aq) + e− ⟶ [Co(NH3)6]2+(aq) is +0.1 V. Calculate the cell potentials to show whether the complex ions, [Co(H2O)6]2+ and/or [Co(NH3)6]2+, can be oxidized to the corresponding cobalt(III) complex by oxygen.
Calculate the equilibriumconstant for the disproportionation of the copper(I) ion atroom temperature:2 Cu+(aq)------>Cu2+(aq) + Cu(s).
Using the dissociation constant, Kd = 7.8 × 10–18, calculate the equilibrium concentrations of Cd2+ and CN– in a 0.250-M solution of Cd(CN)4 2−.
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