Question

Analytical Chemistry Monoprotic weak acid-base equilibrium Hydrolysis. Please show step by step writing instructions on how to solve

Calculate the pH of 0.10 F ethylammonium chloride (CH3CH2NH3C1) (100% soluble salt). The Kh for ethylamine (CH3CH2NH2) is 4.7 x 104. Use the systematic approach to equilibrium to derive in detail the expression you used to calculate either [OH] or [H*].

Answer 1

In aqueous solution, ethylamine undergoes the acid base reaction: H3 C CH ₂ MHz (og) + H204) I CH₃ CH, NO Hz + 8 And we write the equilibrium equation in the usual way: 14 = [Ch CH ny] [on] - CH₂ CH₂ H, (aq)] So, if a miles of ethylamine associate, we can put in some numbers: K . x.x Pritial Concentration of a - 0.10-x Lethylamine a oilor => 22 - x = 4.7 X100 [ Ke or can wear] a 4.7x10 now, it is too sman that orlorne n oilo 322 4.7 x169 => x: 74.7 xH10x164 => x = 0.68x102 Concentration of tot? = 0.68x102 poh = -log (6.68x152 = 2.17 we know, pH + polt - 14 =) PH= 14-2.17 " The ph of oil of Cty Chh stela 11.83. = 11.83