What is the pH of the resulting solution if 95 mL of 0.514 M methylamine, CH3NH2,...
What is the pH of the resulting solution if 30. mL of 0.432 M methylamine, CH3NH2, is added to 15 mL of 0.234 M HCl? Assume that the volumes of the solutions are additive. Ka = 2.70 × 10-11 for CH3NH3+ ?
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...
A chemistry graduate student is given 125. mL of a 0.30 M methylamine (CH3NH2) solution. Methylamine is a weak base with K= 4.4 x 10 . What mass of CH3NH2Cl should the student dissolve in the CH3NH, solution to turn it into a buffer with pH = 10.30? You may assume that the volume of the solution doesn't change when the CH NH2Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2...
A chemistry graduate student is given 125. mL of a 0.10 M methylamine (CH3NH2 solution. Methylamine is a weak base with K,-4.4x 10- . what mass of CH3NH3 Br should the student dissolve in the CH3NH2 solution to turn it into a buffer with pH = 10.50? You may assume that the volume of the solution doesn't change when the CH3NH3 Br is dissolved in it. Be sure your answer has a unit symbol, student dissalve in the CH,NH, solution...
25.4 mL of 0.12 M methylamine (CH3NH2) is titrated with 0.15 M HCI. (a) What is the pH after 14.2 mL of the HCI has been added? (b) What is the pH at the equivalence point in the titration? K(CH3NH2) = 4.4 x 10-4
What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after the addition of 50 mL of a 0.5 mol/L solution of HCl? 5. What is the pH of 50 mL of a 1.0 mol/L methylamine (CH3NH2) solution after the addition of 50 mL of a 0.5 mol/L solution of HCI?
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine, CH3NH2, with 25.00 mL of 0.10 M methylammonium chloride, CH3NH3C1? Assume that the volume of the solutions are additive and that Kb = 3.70 times 10-4 for methylamine. 10.27 10.57 10.87 11.78 Which statement about buffers is true? Buffers have a pH = 7. Buffers consist of a strong acid and its conjugate base. A buffer does not change pH on addition of a...
Calculate the pH of a 1.40 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4. Calculate the pH of a 1.40 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4. 1.61 8.75 5.25 12.39
A chemist titrates 130.0 mL of a 0.0647 M methylamine (CH3NH2 solution with 0.5334 M HNO3 solution at 25 °C. Calculate the pH at equivalence. The p K, of methylamine is 3.36 Round your answer to 2 decimal places Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HNO3 solution added pH =
Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine). The Kb of methylamine is 4.4 × 10−4. can you please show your work and explain the steps on how you get 12.09 as the answer