1. Complete an ICE table and calculate the pH for the following solutions. a. 0.50 M...
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...
Activity #2 Calculate the pH of the following basic solutions. 1. Calculate the pH and pOH of a 0.200 M Ca(OH)2 2. Calculate the equilibrium concentrations for [OH-], [HB+), and [B], the pH and pOH for a 0.200 M pyridine solution. (CsH5N) Kb = 1.4 X 10-9 3. Calculate the equilibrium concentrations for [OH-], [HB], and [B], the pH and pOH for a 0.200 M methylamine. (CH3NH2) Kb = 4.4 X 10-4 4. Calculate the equilibrium concentrations for [OH-], [HB+],...
Find the pH of the following solutions: 1. 0.335 M HC2H3O2 (Ka=1.8*10^-5) 2. 0.417 M CH3NH2 (Kb=4.4*10^-4)
1) Calculate the pH of a 0.026 M solution of NH4NO3. Kb of NH3= 1.8x10^-5. include both the dissociation and hydrolysis equations in the set up 2)calculate the pH of a 75 ml buffer solution containing 0.20 M of citric acid(C6H8O7, Ka= 3.2x10^-7) and 0.30 M sodium citrate. and what is the pH after adding 3.0 mlbof 1.5 M HCl to the buffer solution in that question? 3) what is the pH of 20.00 ml of 0.40 M nitrous acid(...
(3 points) A 0.0730 M solution of a monoprotic acid is 1.07% ionized. What is the pH of the solution? Calculate the Ka of the acid. (2 points) The pH of a 0.025 M solution of a monoprotic acid is 3.21. What is the Ka value for the acid? (2 points) Determine the percent ionization of a 0.0028 M HA solution. (Ka of HA = 1.4 x 10-9) (4 points) Lysine is triprotic amino acid (separately loses three H’s in...
1. Rank the solutions in order of decreasing [H3O+]: 0.10 M HF, 0.10 M HCl, 0.10 M HClO, 0.10 M HC6H5O. 2. The beaker will be filled to the 0.50 L mark with a neutral solution. Set the pH to 3.95 by using the green arrows adjacent to the pH value indicated on the probe in the solution. Once you adjust the pH, note the corresponding OH− ion concentration in M as given in the graphic on the left side...
Calculate the pH of the following solutions 1. A solution that is 6.0×10−2 M in potassium propionate (C2H5COOK or KC3H5O2 ) and 8.5×10−2 M in propionic acid (C2H5COOH or HC3H5O2 ). The Ka of propionic acid is 1.3×10-5. 2. A solution that is 8.0×10−2 M in trimethylamine, (CH3)3N, and 0.12 M in trimethylammonium chloride, (CH3)3NHCl. The Kb of trimethylamine is 6.4×10-5. 3. A solution that is made by mixing 50.0 mL of 0.16 M acetic acid and 50.0 mL of...
1. Calculate the pH of the following solutions. Show all of your work. a. 0.0050 M nitric acid, HNO3 b. 0.50 M hydrocyanic acid, HCN Ka = 4.0 x 10-10 2. A student was given the following problem: Calculate the pH of a 0.50 Mama bromide (NHaBr) solution if the Kb of NH3 is 1.8 x 10. The student provided the fo work. Identify the error(s) and calculate the correct pH. NH; (aq) + H20 (1) = NH3 (aq) +...
thank you Describe how you would calculate the pH of the following 0.10 M aqueous solutions: (a) sodium monohydrogen phosphate (b) glycine hydrochloride (c) trisodium citrate For example: treat as monoprotic acid and use Kai; treat as intermediate form and use Ka, Ka... Find the pH of a solution prepared by dissolving 1.00 g of potassium hydrogen phthalate (204.221 g/mol) and 1.20 g of disodium phthalate (210.094 g/mol) in 50.0 mL of water. (pKai = 2.950, pK2 = 5.408) The...
please help!! calculate pH of solutions on second page a-c!! 1. (4 points) A buffer solution is created with C;H,NH, and 0.012 M C;HsNH2. The K, for C,H,NH2 is 4.7 х 104. What is the concentration of C,HNH, in the buffer solution that has a pH of 11.50? а. What is the concentration of the buffer solution if 0.0011 M HC is added to the buffer in part a.? b. Why is the buffer a basic solution? Could this weak...