Determine the equilibrium concentration of the base HS− given that Kb=1.0×10−7 and the equilibrium concentrations of OH− and H2S are 6.0×10−4 M, and 4.4×10−7 M respectively.
Determine the equilibrium concentration of the base HS− given that Kb=1.0×10−7 and the equilibrium concentrations of...
Determine the equilibrium concentration of the base NH3 given that pKb=4.76 and the equilibrium concentrations of OH− and NH+4 are 6.5×10−5 M, and 0.42 M respectively. Report your answer with two significant figures.
Determine the equilibrium concentration of the base C5H5N given that pKb=8.77 and the equilibrium concentrations of OH− and C5H5NH+ are 0.0032 M, and 4.9×10^−6 M respectively. Report your answer with two significant figures.
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?
From the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb for each of the weak bases. (a) HCH3CO2: [H3O+ ] = 1.53 ✕ 10−3 M, [CH3CO2− ] = 1.53 ✕ 10−3 M, [HCH3CO2] = 0.138 M (b) ClO−: [OH − ] = 2.51 ✕ 10−4 M, [HClO] = 2.51 ✕ 10−4 M, [ClO− ] = 0.250 M
Determine the pK b for the base B given that the equilibrium concentrations are [B]=2.64 M , [ HB + ]=1.5 M , and [ OH − ]=1.2 M .
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?
Determine the pKb for the base B given that the equilibrium concentrations are [B]=1.5 M, [HB+]=0.87 M, and [OH−]=0.75 M. Report your answer with two decimal places.
A certain weak base has a Kb of 8.80×10−7. What concentration of this base will produce a pH of 10.07? concentration: ???? M
A certain weak base has a Kb of 7.00 x 10-7. What concentration of this base will produce a pH of 10.08? concentration: M
The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For the generic weak base, B B(aq)+H2O(l)⇌BH+(aq)+OH−(aq) this constant is given by Kb=[BH+][OH−][B] Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. Percent ionization=[OH−] equilibrium[B] initial×100% Strong bases, for which Kb is very large, ionize completely (100%). For weak bases, the percent ionization changes with concentration. The more dilute the solution, the greater the percent ionization....