Question

Iul See Periodic Table See Hint Calculate the equilibrium concentration of Ag (aq) in a solution that is initially 0.120 M AgNO, and 0.840 MNH3, and in which the following reaction takes place: Ag (aq) + 2NH, (aq) (NH)2(aq) (K - 1.70.10) M Ag

Answer 1

O Agtas) + 2ne13(as) 00120 . 0.840 = Ag Creuz) taey HUB -0.120: - 2X0-120 t00120 O ook 0.120 CS 0 0.6 Kf = 1.7*10* . It's very large value, so we take dessociation of Ag (NH3) 1. Ag (NH3)₂ + = Ast+ 2NH3 kd=t. I 00120 -X + 0.6+2% 0.588 *667. (e) (0.6+2x)? (0-120-4) O x-neglect 00588X607s (0.36) 0.120 l7X107 0.988X10 = *g 0.6 +2x 0.5 % x= 0.120 x0.588 Xo 0.36 88 x6 ²7 3= 0.196 X10'M - The Equilionum Agt (as) is 0-196810*49. Concentration of

7 at 11 270 . Ni (nuogh it Goh [Ni (Nu3b] ** + 2003 (as) Initial Cancen britton of Ni (NO3)2 - Imole = 103 mill mote 1 mill mole = 10-3 mole [mi(oucoz)] = x1000 = 103 x 100 = 0.0037M Anes, Mitast 6MHz ? [Mi (MH3lo] 2t . I 0.0037 0.5 SEO C -0.0037 EX0,0057 +0.0037 E o 0.4978 0.0037 [Nilika djet Z with + 6H3 .. kd = 14 0.0037 0.4778 - -x tx tox 0.0037-x . ta p ab +0,4778 0.1818x68 (X).(64701437e)% 010037-X 0.0034 xosla bla xros (0,4978) * za 0.000679268868 -0.05esxif 0.01189 The Esui librum Concentration of Nit?is = 0.0565X6M R Iz 0.181XLO HU W