Caffeine, C8H10N4O2is a weak base. Determine the value of Kbfor caffeine if a solution at equilibrium has [C8H10N4O2] = 0.050M, [C8H10N4O2H+] = 5 x 10-3 M, and [OH-] = 2.5 x 10-3M
C8H10N4O2(aq) + H2O(l) ⇌ C8H10N4O2H+(aq) + OH-(aq)
Caffeine, C8H10N4O2is a weak base. Determine the value of Kbfor caffeine if a solution at equilibrium...
Question 7 Caffeine, CH 10N4O2 (aq) is a weak base. What is the value of K for caffeine if a solution at equilibrium has [C3H10N 02] = 0.050 M [C8H10N4O2H*]= 5.0 x 10-3M and [OH-] = 2.5 x 10-3M? Write the ionization of caffeine with water and write the Kb expression. Then solve for the kb.
1) The pH of an aqueous solution of 0.442 M caffeine (a weak base with the formula C8H10N4O2) is ______ 2) The hydroxide ion concentration, [OH-], of an aqueous solution of 0.442 M diethylamine (a weak base with the formula (C2H5)2NH) , Kb = 6.9×10-4, is: [OH-] = ________ M.
The pH of an aqueous solution of 0.462 M caffeine (a weak base with the formula C8H10N4O2) is
Caffeine (C8H10N4O2) is a weak base. The pH of a caffeine concentration of 455 mg/L is found to be 7.48. Calculate the pKb of the solution.
Methylamine, CH3NH4, is a weak base. A 0.504 M solution of methylamine has equilibrium concentrations of both CH3NH3^+ and OH^- equal to 0.0150 M. What is the Kb of the base? CH3NH2(aq) + H2O(l) <> CH3NH3^+(aq) + OH^-(aq)
Caffeine (C8H10N4O2) is a weak base with a pKb of 10.4. Calculate the pH of a solution containing a caffeine concentration of 460 mg/L . Express your answer to one decimal place.
Caffeine (C8H10N4O2) is a weak base with a pKb of 10.4. Calculate the pH of a solution containing a caffeine concentration of 156 mgL−1 . Express your answer to one decimal place.
Caffeine (C8H10N4O2) is a weak base with a pKb of 10.4. Part A Calculate the pH of a solution containing a caffeine concentration of 281 mgL−1 . Express your answer to one decimal place.
please explain! thank you! 13. (4 pts) Caffeine, a stimulant in coffee and tea, is a weak base that ionizes in water according to the equation. A 0.15 M solution of caffeine has a pH of 8.45. What is the Ko of caffeine. CHNO2(aq) + H2O(l) = HCHON 02 (aq) + OH(aq) A) 8.4 x 10-17 B) 5.3 x 10-11 C) 1.6 x 10 D) 0.013 E) 0.187 11 TL
This question pertains to the pH of a weak acid/weak base salt combo. For an aq solution of NH4NO2, these are the combinations of reactions that are possible. (1) NH4+(aq) + NO21-(aq) ⇆ NH3(aq) + HNO2(aq)____________K1 = ? (2) NH4+(aq) + H2O(l) ⇆ H3O+(aq) + NH3(aq)_______________Ka = 5.6 x 10-10 (3) NO21- + H2O(l) ⇆ HNO2(aq) + OH-(aq)_________________Kb = 2.2 x 10-11 (4) 2H2O(l) ⇆ H3O+(aq) + OH-(aq)_________________________Kw =1.0 x 10-14 Write the symbolic expression for the equilibrium constants...