What is the pH of a 0.14 M solution of methylammonium chloride, CH NH, CI? What is the concentration of methylamine...
8. What is the pH of a 0.25 Maqueous solution of methylamine hydrochloride, CH,NH,CI? K, for methylamine CH3NH2 is 4.4 x 104
Calculate the pH and concentrations of CH NH, and CH NH; in a 0.0293 M methylamine (CH, NH,) solution. The Kb of CH3NH, is 4.47 x 10-4. pH = [CH, NH] = [CH, NH}=
A chemistry graduate student is given 450. mL of a 0,60 M methylamine (CH NH, solution, Methylamine is a weak base with of CH NH,Br should the student dissolve in the CH, NH, solution to turn it into a buffer with pH - 11.09 4.4 x 10 What mass You may assume that the volume of the solution doesn't change when the CH, NH Br is dissolved in it. Be sure your answer has a unit symbol, and round it...
A solution is prepared at 25 °C that is initially 0.19 Min methylamine (CH2NH2), a weak base with K; = 4.4 x 10 +, and 0.43 Min methylammonium bromide (CH NH Br). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 1 x 6 ?
what is the pH of 0.36M methylamine solution? pH of 0.36 M methylamine sol. (Kb = 4.4 * 10^-4)
A buffered solution containing dissolved aniline, CH NH, and aniline hydrochloride, CH-NH, CI, has a pH of 5.49. A. Determine the concentration of CGH NH; in the solution if the concentration of CoH_NH, is 0.290 M. The pKy of aniline is 9.13. [C,H,NH] = M B. Calculate the change in pH of the solution, ApH, if 0.358 g NaOH is added to the buffer for a final volume of 1.55 L. Assume that any contribution of NaOH to the volume...
A buffered solution containing dissolved aniline, CH,NH, and aniline hydrochloride, CH NH, CI, has a pH of 5.48. A. Determine the concentration of CH NH in the solution if the concentration of C, H,NH, is 0.320 M. The pKb of aniline is 9.13. [C,H, NH] = B. Calculate the change in pH of the solution, ApH, if 0.390 g NaOH is added to the buffer for a final volume of 1.65 L. Assume that any contribution of NaOH to the...
A buffer solution contains 0.311 MCH, NH,CI and 0.362 M CHANH, (methylamine) Determine the pH change when 0.098 mol HBr is added to 1.00 L of the buffer. pH after addition - pH before addition pH change
5.83 is wrong
Calculate the pH at the equivalence point for the titration of 0.110 M methylamine (CH,NH,) with 0.110 M HCI. The Ky of methylamine is 5.0 x 10- pH = 5.83
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...