Question

Find the pH of the following solutions in equilibrium with 10-4 atm ammonia. Show all calculations. Assume an open system.

            a. distilled water                     b. 10^-2 M NH₄Cl

please apply Henry's Law

Answer 1

Comment in case of any doubt.

=) solution atm ous ta th al 1. According to Henry's Law: c = Kt Pt partial pressure . concentration above Henry's in aqueous low 1 KH of NH₃ solution constant ALNHIF 5.88103 M This concentration of the we occurs. (a) to do in the (a) In distilled water solution, even if any reaction following a equilibruin will 1. decide phi (for Nil final (NH2) = 5.8x10M, so if rm NH3 is used then ENHA ICE NH₃ lags + H2Old) t Nhut (ar) + OH(aq), k, =18x105 Ii c: -alsay) E: 5.8x102 in This will be maintained by more WHz dissolving in solution (from above) despite some NH3 used. ď above reactions Wow exrös kis IN HUILOH] = (M)0) 213 - x²= 1.8x10 x [NH₃ 58x103 5.8x103 58x103 =) = 3.2318159 M=COH] [H3O+] = 10l4 Toy Coho - 3:23),xjõ4 = 3.095 x16" pH = -log(Hot) = -log (3.095 x16") = (10.5] Answer ☺ As found above. CNPJ = 518x1oCM; given CN H1y60]= 10CM This is a buffer whose pH can be found using Henderson - Hasselbalch equation as follows: pH = pka + long and the = -log(1-xia®) + hogy a sign one) no (NACO = 14.51 Ansumer wa