Caffeine is a weak base with a Kb of 4.1×10−4. Calculate the initial molar concentration of...

Question

Question

Caffeine is a weak base with a Kb of 4.1×10−4.

Calculate the initial molar concentration of a solution of caffeine if the pH is 10.42.

Answer 1

Answer #1

Kb for caffeine (B) = 4.1 x 10-4 Given pH = 10.42 pOH = 14 - pH = 14 – 10.42 = 3.58 Caffeine in water is B + H2O ---------> B

Answer 2

Similar Homework Help Questions

Ammonia is a weak base with a Kb of 1.8×10^−5 Calculate the initial molar concentration of...

Ammonia is a weak base with a Kb of 1.8×10^−5 Calculate the initial molar concentration of a solution of ammonia if the pH is 10.48. I got .0051 but it is incorrect. Ammonia is a weak base with a Kb of 1.8 x 10 5. Calculate the initial molar concentration of a solution of ammonia if the pH is 10.48. concentration: 1.0051
Ammonia is a weak base with a Kb of 1.8 x 10-5. Calculate the initial molar...

Ammonia is a weak base with a Kb of 1.8 x 10-5. Calculate the initial molar concentration of a solution of ammonia if the pH is 11.00. concentration: M
Calculate the pH of a 0.26M methylamine solution? (weak base)

a. Calculate the pH of a 0.26M methylamine solution? (weak base)b. Consider the following three solutions of equal concentration. Rank the three solutions from most basic to least basic based on their Kb: (a) aniline 4.3 x 10-10, (b) methylamine5.0× 10–4, (c) caffeine 4.1 x 10-4.

Caffeine (C8H10N4O2) is a weak base. The pH of a caffeine concentration of 455 mg/L 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.
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4)...

A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ? [CH3NH2]equilibrium = ? M [CH3NH3+ ]equilibrium = ? M B)Calculate the pH of a 0.0115 M aqueous solution of nitrous acid (HNO2, Ka= 4.6×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = ? [HNO2]equilibrium = ? M [NO2- ]equilibrium = ? M C)...
1) The pH of an aqueous solution of 0.442 M caffeine (a weak base with the...

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.

A 250.0 mL solution contains two weak bases, pyridine (Kb = 1.7 x 10^-9) and caffeine...

A 250.0 mL solution contains two weak bases, pyridine (Kb = 1.7 x 10^-9) and caffeine (Kb = 4.1 x 10^-4). This solution contains 1.00 x 10^-3 mol of each of the bases. What's the pH of this solution?
Caffeine is a very weak monobasic Bronsted base, with Kb = 4 x 10-14. Spectroscopic and...

Caffeine is a very weak monobasic Bronsted base, with Kb = 4 x 10-14. Spectroscopic and computational studies show that the proton most likely attaches on the imine nitrogen (–N=). Given this information, sketch the protonated form (A) and deprotonated form (B) of caffeine below, and indicate the regions of stability of each form as a function of pH on the chart from 0 to 14
Caffeine (C8H10N4O2) is a weak base with a pKb of 10.4. Calculate the pH of a...

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 concentrati...

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.