How is the Kb value related to the [OH−] at equilibrium?*1 pointThe larger the Kb the higher the [OH−].The smaller the Kb the higher the [OH−].The larger the Kb the lower the [OH−].The smaller the Kb the [OH−] remains constant.

Give any two characteristics of equilibrium constant (kc or kP)

For the dissolving of Mn(OH)2, the equilibrium constant expression, Ksp, is Question 7Select one:Ksp = [Mn2+] [OH-]2 / [Mn(OH)2]Ksp = [Mn2+] [OH-] / [Mn(OH)2]Ksp =  [Mn(OH)2]  / ([Mn2+] [OH-] 2) Ksp = [Mn2+] [OH-]2Ksp = [Mn2+] [OH-]

Consider the following elementary reaction:NO2(g) +O3(g) →NO3(g) +O2(g)Suppose we let k1 stand for the rate constant of this reaction, and k−1 stand for the rate constant of the reverse reaction.Write an expression that gives the equilibrium concentration of O3 in terms of k1, k−1, and the equilibrium concentrations of NO2, NO3, and O2.

How is the equilibrium constant (K) calculated?Question 4Select one:a.[products][reactants][products][reactants]b.[reactants][products][reactants][products]c.[reactants] + [products]d.[products] x [reactants]

What does a Ka value of approximately 1 show about the equilibrium?A.The acid has completely dissociated.B.The solution can act as both an acid and a base.C.Very little of the acid has dissociated.D.Some of the acid has dissociated.