At 40.0 C, pKa for the conjugate acid diethylamine, (C2H5)2NH IS 11.02 . A. Write the...
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 40.0 C be equal to -6.3 kJ if [(C2H5)2nh]= 0.00443 M and [(C2H5)2NH2^+]= 0.00482 m?
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At 40.0 C, pKa for the conjugate acid diethylamine, (C2H5)2NH IS
11.02
. A. Write the...
Diethylamine ((C2H5)2NH) is a weak base. In aqueous solution at 25°C, it reacts with water to...
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
(1) Given the following information: hydrocyanic acid HCN Ka = 4.0×10-10 diethylamine (C2H5)2NH Kb = 6.9×10-4...
(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?...
Determine the pH during the titration of 31.1 mL of 0.259 M diethylamine ((C2H5)2NH, Kb 6.9x10) by 0.259 M HI at the fo...
Determine the pH during the titration of 31.1 mL of 0.259 M diethylamine ((C2H5)2NH, Kb 6.9x10) by 0.259 M HI at the following points (Assume the titration is done at 25 °C) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HI (b) After the addition of 12.9 mL of HI (c) At the titration midpoint (d) At the equivalence point (e) After adding 48.5 mL of HI
Determine the pH...
pKa Conjugate base Acid formula Conjugate base name Acid name F3CCOOH 0.20 F3ccoo trifluoroacetic acid trifluoroacetate...
pKa Conjugate base Acid formula Conjugate base name Acid name F3CCOOH 0.20 F3ccoo trifluoroacetic acid trifluoroacetate ion 13.80 Cl3CCOOH 13.34 0.66 Cl3CCOO trichloroacetic acid trichloroacetate ion HOOCCOOH 1.23 HOOCCOO oxalic acid hydrogen oxalate ion 12.77 Cl2HCCOOH 12.70 dichloroacetic acid 1.30 Cl2HCCOO dichloroacetate ion H2SO3 12.23 1.77 HSO3 sulfurous acid hydrogen sulfite ion 1.92SO42- HSO4 hydrogen sulfate ion sulfate ion 12.08 HCIO2 1.95 CI02 chlorous acid chlorite ion 2.12 H2PO.4 phosphoric acid H3PO dihydrogen phosphate ion 11.88 CIH2CCOOH 2.87 CIH2CCOO 11.13...
1 a) Write the aqueous acid dissociation reactions for an acid and base dissociation reaction for a base according to th...
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...
1. A weak acid (benzoic acid) is titrated with a strong base such as sodium hydroxide....
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...
1. Calculate the pH at 25°C of a 0.757 M solution of a weak acid that...
1. Calculate the pH at 25°C of a 0.757 M solution of a weak acid that has Ka = 9.28 x 10 2. Determine the Kb of a weak base if a 2.50 M solution of the base has a pH of 9.595 at 25°C. 3. The overall dissociation of malonic acid, H2C3H2O4, is represented below. The overall dissociation constant is also indicated. H2C3H204 = 2 H+ + C3H2042- K = 3.0 x 10-9 To a 0.025-molar solution of malonic...
56,57,58,59,60,61,62 56) For the reaction 3H2(g) + N2(g)s-2NH(g), determine the equilibrium constant at 600°C if at this temperature, the equilibrium concentrations are: [N2 453 M; H:-2.49 M and [...
56,57,58,59,60,61,62
56) For the reaction 3H2(g) + N2(g)s-2NH(g), determine the equilibrium constant at 600°C if at this temperature, the equilibrium concentrations are: [N2 453 M; H:-2.49 M and [NHs] 7.62 M 57) When a sample of aqueous hydrochloric acid was neutralized with aqueous sodium hydroxide in a calorimeter, the temperature of 100.0 g of water surrounding the reaction increased from 25.0°C to 31.50. If the specific heat of water is 1.00 calV(g.°C), calculate the quantity of energy in calories involved...
Phenol, the active ingredient in Chloraseptic throat spray, is a monoprotic weak acid whose formula is...
Phenol, the active ingredient in Chloraseptic throat spray, is a monoprotic weak acid whose formula is HC6H5O (Ka = 1.3 * 10-10). Suppose 12.50 g of phenol is dissolved in water and enough water is added to bring the total solution volume to 250.0 mL. Write the balanced chemical equation for the resulting equilibrium. Identify all conjugate acid/ base pairs. (b) Calculate the molarities of all species in the equilibrium mixture, the percent dissociation of phenol, and the pH of...
1. Write the equilibrium expression for the autoionization of water. Using this expression define the terms...
1. Write the equilibrium expression for the autoionization of water. Using this expression define the terms acid and base and pH. 2. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 0.082M solution of triethylamine. 3. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 1.570 M solution of hydrogen cyanide. 4. The acid-dissociation constant for hypochlorus acid is 3.0 X 10-8. Calculate the concentrations of H3O+, CIO-, and HCIO at equilibrium if the initial concentration...
Determine the pH during the titration of 31.1 mL of 0.259 M diethylamine ((C2H5)2NH, Kb 6.9x10) by 0.259 M HI at the following points (Assume the titration is done at 25 °C) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HI (b) After the addition of 12.9 mL of HI (c) At the titration midpoint (d) At the equivalence point (e) After adding 48.5 mL of HI
Determine the pH...
pKa Conjugate base Acid formula Conjugate base name Acid name F3CCOOH 0.20 F3ccoo trifluoroacetic acid trifluoroacetate ion 13.80 Cl3CCOOH 13.34 0.66 Cl3CCOO trichloroacetic acid trichloroacetate ion HOOCCOOH 1.23 HOOCCOO oxalic acid hydrogen oxalate ion 12.77 Cl2HCCOOH 12.70 dichloroacetic acid 1.30 Cl2HCCOO dichloroacetate ion H2SO3 12.23 1.77 HSO3 sulfurous acid hydrogen sulfite ion 1.92SO42- HSO4 hydrogen sulfate ion sulfate ion 12.08 HCIO2 1.95 CI02 chlorous acid chlorite ion 2.12 H2PO.4 phosphoric acid H3PO dihydrogen phosphate ion 11.88 CIH2CCOOH 2.87 CIH2CCOO 11.13...
1. Calculate the pH at 25°C of a 0.757 M solution of a weak acid that has Ka = 9.28 x 10 2. Determine the Kb of a weak base if a 2.50 M solution of the base has a pH of 9.595 at 25°C. 3. The overall dissociation of malonic acid, H2C3H2O4, is represented below. The overall dissociation constant is also indicated. H2C3H204 = 2 H+ + C3H2042- K = 3.0 x 10-9 To a 0.025-molar solution of malonic...
56,57,58,59,60,61,62
56) For the reaction 3H2(g) + N2(g)s-2NH(g), determine the equilibrium constant at 600°C if at this temperature, the equilibrium concentrations are: [N2 453 M; H:-2.49 M and [NHs] 7.62 M 57) When a sample of aqueous hydrochloric acid was neutralized with aqueous sodium hydroxide in a calorimeter, the temperature of 100.0 g of water surrounding the reaction increased from 25.0°C to 31.50. If the specific heat of water is 1.00 calV(g.°C), calculate the quantity of energy in calories involved...
1. Write the equilibrium expression for the autoionization of water. Using this expression define the terms acid and base and pH. 2. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 0.082M solution of triethylamine. 3. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 1.570 M solution of hydrogen cyanide. 4. The acid-dissociation constant for hypochlorus acid is 3.0 X 10-8. Calculate the concentrations of H3O+, CIO-, and HCIO at equilibrium if the initial concentration...
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