Question

Enter your answer in the provided box. Calculate the pH of a 0.25 M methylamine solution. pH =

Answer 1

= CH₃NH₂ + H2O 0.25M (initial) CM₂ NH3t ton 0 0 0.250 0.25% 0.2501-4) Kb = (0,250) (0.250) = 0.25x² 0.25(1-x) 1-da 1 (since & is very small for weak berse) kb for methylamine = 4:48 104 [literature search] 4.48 164 = 0.25x²

x²= 4.4x154 = 17.6x104 0.25 d= (17.6 x 10-4) "? 1 : 4.20 X 100 [or" ] = 0.258 = 0.25 X4.20x10*M = 1.05X16X Since; Po H = -logo Tour] =-legno (105 X 10%) = 1.98 As we know; PH+ Por = 14 PH = 14-POH = 14 -1.98 - 12.02