Diethylamine ((C2H5)2NH) is a weak base. In aqueous solution at
25°C, it reacts with water to produce its conjugate acid, the
diethylammonium ion ((C2H5)2NH2+), and the hydroxide ion (OH
−).
(a) If the base-dissociation constant (Kb) of diethylamine is
7.0 ✕ 10−4, calculate the acid-dissociation constant (Ka) for the
conjugate acid.
(b) What are the corresponding pKa and pKb values for this
conjugate acid-base pair?
pKa
pKb
Diethylamine ((C2H5)2NH) is a weak base. In aqueous solution at 25°C, it reacts with water to...
At 40.0 C, pKa for the conjugate acid diethylamine, (C2H5)2NH IS 11.02 . A. Write the balanced chemical equation for the dissociation of diethylamine in water. B. Calculate Kb at 40.0 C for diethylamine. Kw is 3.0 X10^-14 at 40.0 C C. Calculate delta G standard at 40.0 C for the dissociation of diethylamine in water. D. What is delta G at 40.0 C when [(C2H5)2NH] = 0.285 m, [OH-]= 0.00989 m? E. At what pH will delta G at...
The hydronium ion concentration of an aqueous solution of 0.461 M diethylamine (a weak base with the formula (C2H5)2NH) is [H3O+] = _____M. The hydroxide ion concentration, [OH-], of an aqueous solution of 0.461 M trimethylamine (a weak base with the formula (CH3)3N) is ____M.
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.
(1) Given the following information: hydrocyanic acid HCN Ka = 4.0×10-10 diethylamine (C2H5)2NH Kb = 6.9×10-4 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.152 M aqueous hydrocyanic acid and diethylamine are mixed. It is not necessary to include states such as (aq) or (s). (2) At equilibrium will the reactants or products be favored? (3) Will the pH of the resulting solution be greater than, less than, or roughly equal to 7?...
In aqueous solution, the azide ion, N3−, is a weak base that accepts a proton from water to form the hydroxide ion, OH −, and hydrazoic acid, HN3, according to the following equation. N3−(aq) + H2O(l) equilibrium reaction arrow OH −(aq) + HN3(aq) The base-dissociation constant (Kb) for this base is 4.04 ✕ 10−10. If a 0.082 M solution of azide ions is prepared, what is the final pH of the solution? (Assume that the temperature is 25°C.)
1 a) Write the aqueous acid dissociation reactions for an acid and base dissociation reaction for a base according to the Bronsted-Lowry definition b) Determine conjugate bases of acids and acids of bases c) Write the equilibrium expression for an acid or a base aqueous dissociation d) Evaluate strength of an acid or base based on its Ka or Kb or pKa or pKb. e) Apply Kw at 25oC and at different temperatures. f) Solve for the pH of strong...
a)Calculate the pH of a weak base solution ([B]0 > 100 • Kb). Close Problem Calculate the pH of a 0.289 M aqueous solution of triethanolamine (C6H15O3N, Kb = 5.8×10-7) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C6H15O3N]equilibrium = M [C6H15O3NH+]equilibrium = M b) Calculate the pH of a 0.0338 M aqueous solution of dimethylamine ((CH3)2NH, Kb = 5.9×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ...
1. A weak acid (benzoic acid) is titrated with a strong base such as sodium hydroxide. Determine the pH at the half equivalence point of the titration. The Ka of the weak acid is 6.3 x 10-5. 2.Calculate the pH of a buffer made from 0.6 M HNO2 and 0.5 M NaNO2. Ka = 4.5 x 10-5 pKa = 4.3 Answer with one digit after the decimal place (e.g. 2.1) Hint: HNO2 is a weak acid. NaNO2 forms the conjugate...
Chapter 16 Relating pKa and pKb Review I Constants | Periodic Table Ar Learning Goal: To understand the relation between the strength of an acid or a base and its pKa and pKb values. The degree to which a weak acid dissociates in solution is given by its acid-ionization constant, Ka. For the generic weak acid, HA, HA(aq) A (aq) H (aq) and the acid-ionization constant is given by a HA Similarly, the degree to which a weak base reacts...
A chemist prepared aqueous solutions of two weak acids: solution A is butyric acid (HC3H8CO2), and solution B is nitrous acid (HNO2). At 25°C, the acid-dissociation constant (Ka) for butyric acid is 1.5 ✕ 10−5 and the base-dissociation constant (Kb) for the nitrite ion (NO2−) is 1.8 ✕ 10−11. Determine the following. (a) the Ka value for nitrous acid (HNO2) (b) the Kb value for the butyrate ion (C3H8CO2−)