C6H5COOH(aq) + S^2- (aq) <------------> C6H5COO^- (aq) + HS^- (aq)
The rate of forward reaction = Kf[C6H5COO]{S^2-]
The react of reverse reaction = Kb[C6H5COO^-][HS^-]
At equilibrium rate of forward reaction is equal to rate of reverse reaction
forward reaction = rate of reverse reaction
Kf[C6H5COO]{S^2-] = Kb[C6H5COO^-][HS^-]
Kf/Kb = [C6H5COO^-][HS^-]/[C6H5COO]{S^2-]
Koverall = [C6H5COO^-][HS^-]/[C6H5COO]{S^2-] [K overall = kKf/Kb]
Using this table of ionization constants, calculate the overall equilibrium constant, Koval CH,COOH(aq) + S?-(aq) =...
Using this table of ionization constants, calculate the overall equilibrium constant, Koverall, for the reaction. HF(aq) + Co - (aq) = F (aq) + HCO3(aq) Koverall =
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Write the acid ionization constants ( also referred to as the equilibrium constant for a weak acid) for the following reactions: a. H2CO3(aq) + H2O(l) H3O+(aq) + HCO3-(aq) b. H2S(aq) + H2O(l) H3O+ (aq) + HS-(aq) c. HC3H5O3 + H2O(l) H3O+(aq) + C3H5O3(aq)
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?
a. Using the initial concentration of CH,COOH (from Problem 3) and the equilibrium concentration of H,0 calculated (from Problem 4), complete the reaction table for vinegar. Ignore the column under H:O() (shaded in gray). Don't forget to write a sign (+ or -) for the "Change” row entry. (9 pts: each entry is 1 pt.) Reaction Table CH.COOH (aq) + H20(0) CH,COO (aq) + H2O (ag) Initial Change Equilibrium b. By using the concentration values at equilibrium in the reaction...
Cd2+ forms two complexes with acetate, with the given overall formation constants. 1. Cd2+ (aq) + CH, CO2 (aq) = Cd(CH, CO2)+(aq) K1 = B1 = 85 2. Cd2 + (aq) + 2 CH, CO2 (aq) = Cd(CH, CO2)2(aq) B2 = 1400 Find the stepwise formation constant, K2, for the reaction 3. Cd(CH, CO2)+ (aq) + CH, CO2 (aq) = CH(CH, CO2)2 (aq) K2 =? K2 = Cd(CIO2)2 and 0.220 mol CH, CO Na. Calculate the fraction of You prepare...