1.
Calculate the pH of a 0.543 M aqueous solution of codeine (C18H21O3N, Kb = 8.9×10-7).
pH =
2. Calculate the pH of a 0.1250 M aqueous
solution of piperidine
(C5H11N, Kb =
1.3×10-3).
pH =
3. Calculate the pH of a 0.0774 M aqueous
solution of the weak base triethylamine
((C2H5)3N,
Kb = 5.20×10-4).
pH =
1. Calculate the pH of a 0.543 M aqueous solution of codeine (C18H21O3N, Kb = 8.9×10-7)....
a. Calculate the pH of a 0.205 M aqueous solution of aniline (C6H5NH2, Kb = 7.4×10-10) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C6H5NH2]equilibrium = M [C6H5NH3+]equilibrium = M b. Calculate the pH of a 0.0555 M aqueous solution of piperidine (C5H11N, Kb = 1.3×10-3) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C5H11N]equilibrium = M [C5H11NH+ ]equilibrium = M
Salt of a Weak Base and a Strong Acid. pH of Solution. Calculate the pH of a 1.19 M aqueous solution of triethylamine hydrochloride ((C2H5)3NHCI) (For triethylamine, (C2H5)3N, Kb = 4.00x 10-4.) Give two decimal places in your answer.
1)In the laboratory, a general chemistry student measured the pH of a 0.405 M aqueous solution of aniline, C6H5NH2 to be 9.254. Use the information she obtained to determine the Kb for this base. Kb(experiment) = 2) In the laboratory, a general chemistry student measured the pH of a 0.405 M aqueous solution of codeine, C18H21O3N to be 10.793. Use the information she obtained to determine the Kb for this base. Kb(experiment) = 3) The hydroxide ion concentration, [OH-], of...
1. Calculate the pH of a 0.0162 M triethylamine hydrochloride solution. Kb ((C2H5)3N) = 5.6 × 10−4. show work. 2. In a flask, you have 35.00 mL of 0.140 M acetic acid, a weak monoprotic acid with Ka = 1.8 × 10−5. Calculate the pH after the addition of 9.10 mL of 0.140 M NaOH. show work.
1)In the laboratory, a general chemistry student measured the pH of a 0.360 M aqueous solution of triethylamine, (C2H5)3N to be 12.120. Use the information she obtained to determine the Kb for this base. Kb(experiment) = 2)In the laboratory, a general chemistry student measured the pH of a 0.360 M aqueous solution of aniline, C6H5NH2 to be 9.198. Use the information she obtained to determine the Kb for this base. Kb(experiment) =
1. Calculate the pH of a 0.447 M aqueous solution of aniline (C6H5NH2, Kb = 7.4×10-10). 2. Calculate the pH of a 0.0590 M aqueous solution of the weak base caffeine (C8H10N4O2, Kb = 4.10×10-4). 3. Calculate the percent ionization of a 0.545 M solution of hydrocyanic acid.
1. What is the pOH of an aqueous solution of 0.171 M hydrobromic acid? pOH = 2. What is the pH of an aqueous solution of 1.77×10-2 M nitric acid? pH = 3. What is the pOH of an aqueous solution of 3.08×10-2 M potassium hydroxide? pOH = 4. What is the pH of an aqueous solution of 3.08×10-2 M potassium hydroxide? pH = 5. Calculate the pH of a 0.409 M aqueous solution of nitrous acid (HNO2, Ka =...
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)...
What is the ph of a 0.050 M triethylamine (C2H5) 3N solution? kB for triethylamine is 5.3 x 10^-4 5.32 2.31 1.30 8.68 or 11.69
a. The hydroxide ion concentration, [OH-], of an aqueous solution of 0.331 M ethylamine (a weak base with the formula C2H5NH2) , Kb = 4.3×10-4, is: [OH-] = ___________ b. The hydronium ion concentration of an aqueous solution of 0.331 M codeine (a weak base with the formula C18H21O3N) is ... [H3O+] = __________