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If the a mixture of methylamine (CH3NH2, pkb = 3.32) in water produces a pH of...
If the a mixture of methylamine (CH3NH2, p Kb = 3.32) in water produces a pH...
If the a mixture of methylamine (CH3NH2, p Kb = 3.32) in water produces a pH of 11.8, what is the initial molar concentration of methylamine in the solution? O A 2.6x10-4M O B 7.7x10-2M O c 3.4x10-5M O D 8.3x10-2M Triethylamine (C2H5)3N) has a pKb = 3.25. What is the value of the equilibrium constant K for this reaction: (C2H5)3NH(aq) + H2O(1) = (C2H5)3N(aq) + H3O+(aq)? O A 1.77x10-11 O B 5.62x10-4 o C More information is needed to...
please explain If the a mixture of methylamine in water produces a pH of 11.2, what...
please explain
If the a mixture of methylamine in water produces a pH of 11.2, what is the concentration of methylamine in the solution? HOC-NH2 + HO Hoc Noth methenemine methylumine) methylammonium ion pk, 10.7 O A 5x10-3M o B 2.5x 10-3M O C 1210-2M O 5x10 M
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution 2...
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution 2 points after the addition of 50 mL of a 0.5 mol/L solution of HCI? Your answer O BE
Calculate the pH of a solution consisting of 0.225 M solution of CH3NH2 (methylamine) and 0.200...
Calculate the pH of a solution consisting of 0.225 M solution of CH3NH2 (methylamine) and 0.200 M CH3NH2 tor (methylammonium chloride). Report answer to 2 decimal places. Kb CH3NH2) - 44 x 10-4 CH3NH2 (aq) + H200 + CH3NH3 (2) + OH(aq) Assuming equal initial concentrations of the given species, which of the following is the weakest acid in aqueous solution? O. HB Ky = 2.0 x 10-6 OB.HD K = 6.0 x 10-2 ОС: НЕ Kg = 4.0 x...
Measure pH of the mixture solution of s ml of 10 Macetic acid and 2 mL...
Measure pH of the mixture solution of s ml of 10 Macetic acid and 2 mL of 1.0 M NaC,H,O, Measured pH: 3.4Y Calculated [H,0*) - Calculations (give setups): Initial molar concentration of HC,H,02: Initial molar concentration of CH,0;": H,O + HC,H,O2 = H,0* + CH20;- Initial Change (Equilibrium] Write the equilibrium constant expression for the above equation. Calculate the experimental ionization constant, K, of acetic acid.
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...
I didn't know which one so I posted all of what I was provided Acid/Base Ionization...
I didn't know which one so I
posted all of what I was provided
Acid/Base Ionization Constants at 25 °C Acid Formula Kal Ka2 Каз Acetic acid CH3COOH 1.8x10-5 Acetylsalicylic acid (aspirin) HC,H-04 3.0x10-4 Aluminum ion Al(H20)43+ 1.2x10-5 Arsenic acid H3 AsO4 2.5x10-4 5.6x10-8 3.0x10-13 Ascorbic acid H2C6H606 7.9x10-5 1.6x10-12 Benzoic acid CH3COOH 6.3x10-5 Carbonic acid H2CO3 4.2x10-7 4.8x10-11 Ferric ion Fe(H20)63+ 4.0*10-3 Formic acid HCOOH 1.8x104 Hydrocyanic acid HCN 4.0*10-10 Hydrofluoric acid HF 7.2x104 Hydrogen peroxide H202 2.4x10-12 Hydrosulfuric...
yes, which the data for the experiment is given in the pictures Problem #1 Use this...
yes, which the data for the experiment is given in the
pictures
Problem #1 Use this data to calculate Ksp of Ca(OH)2. The Ca(OH) used was 15.0 ml, titrated with 0.05M HCI DATA TABLE: TITRATION OF THE SUPERNATANT LIQUID Trial 1 Trial 2 Data Volume of CaOH, solution, mL (supernatant liquid) Initial buret reading, mL Final buret reading, mL Volume of HCl required for titration, mL Equivalence point (mL) Average Kop Problem #2 R PPPPPP LABORATORY REPORT YOU MUST SHOW...
If the a mixture of methylamine (CH3NH2, p Kb = 3.32) in water produces a pH of 11.8, what is the initial molar concentration of methylamine in the solution? O A 2.6x10-4M O B 7.7x10-2M O c 3.4x10-5M O D 8.3x10-2M Triethylamine (C2H5)3N) has a pKb = 3.25. What is the value of the equilibrium constant K for this reaction: (C2H5)3NH(aq) + H2O(1) = (C2H5)3N(aq) + H3O+(aq)? O A 1.77x10-11 O B 5.62x10-4 o C More information is needed to...
please explain
If the a mixture of methylamine in water produces a pH of 11.2, what is the concentration of methylamine in the solution? HOC-NH2 + HO Hoc Noth methenemine methylumine) methylammonium ion pk, 10.7 O A 5x10-3M o B 2.5x 10-3M O C 1210-2M O 5x10 M
5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution 2 points after the addition of 50 mL of a 0.5 mol/L solution of HCI? Your answer O BE
Calculate the pH of a solution consisting of 0.225 M solution of CH3NH2 (methylamine) and 0.200 M CH3NH2 tor (methylammonium chloride). Report answer to 2 decimal places. Kb CH3NH2) - 44 x 10-4 CH3NH2 (aq) + H200 + CH3NH3 (2) + OH(aq) Assuming equal initial concentrations of the given species, which of the following is the weakest acid in aqueous solution? O. HB Ky = 2.0 x 10-6 OB.HD K = 6.0 x 10-2 ОС: НЕ Kg = 4.0 x...
Measure pH of the mixture solution of s ml of 10 Macetic acid and 2 mL of 1.0 M NaC,H,O, Measured pH: 3.4Y Calculated [H,0*) - Calculations (give setups): Initial molar concentration of HC,H,02: Initial molar concentration of CH,0;": H,O + HC,H,O2 = H,0* + CH20;- Initial Change (Equilibrium] Write the equilibrium constant expression for the above equation. Calculate the experimental ionization constant, K, of acetic acid.
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...
I didn't know which one so I
posted all of what I was provided
Acid/Base Ionization Constants at 25 °C Acid Formula Kal Ka2 Каз Acetic acid CH3COOH 1.8x10-5 Acetylsalicylic acid (aspirin) HC,H-04 3.0x10-4 Aluminum ion Al(H20)43+ 1.2x10-5 Arsenic acid H3 AsO4 2.5x10-4 5.6x10-8 3.0x10-13 Ascorbic acid H2C6H606 7.9x10-5 1.6x10-12 Benzoic acid CH3COOH 6.3x10-5 Carbonic acid H2CO3 4.2x10-7 4.8x10-11 Ferric ion Fe(H20)63+ 4.0*10-3 Formic acid HCOOH 1.8x104 Hydrocyanic acid HCN 4.0*10-10 Hydrofluoric acid HF 7.2x104 Hydrogen peroxide H202 2.4x10-12 Hydrosulfuric...
yes, which the data for the experiment is given in the
pictures
Problem #1 Use this data to calculate Ksp of Ca(OH)2. The Ca(OH) used was 15.0 ml, titrated with 0.05M HCI DATA TABLE: TITRATION OF THE SUPERNATANT LIQUID Trial 1 Trial 2 Data Volume of CaOH, solution, mL (supernatant liquid) Initial buret reading, mL Final buret reading, mL Volume of HCl required for titration, mL Equivalence point (mL) Average Kop Problem #2 R PPPPPP LABORATORY REPORT YOU MUST SHOW...
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