Modify Figure 8-7 to find the concentrations of species in 0.05 M NH3. The only change required is the value of F. How do the pH and fraction of ammonia hydrolysis (= [NH⁺₄ ]/([NH⁺₄ ] + [NH₃])) change when the formal concentration of NH₃ increases from 0.01 to 0.05 M?

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А В C E Using Goal Seek for Ammonia Equilibrium pKb = 4.755 Kb = 1.76E-05 = 10^-B3 4 pKw = 14.00 Kw = 1.00E-14 10^-B4 %3D F = 0.01 7 pH = Initial value is estimate 8 [H*] = 1.00E-09 10^-B7 9. [NH4*] = Kw/[H*] - [H*] = 1.00E-05= D4/B8-B8 10 [OH] = Kw[H*] = 1.00E-05 = D4/B8 [NH3] = F - Kw[H*] + [H*] = Q = [NH4*][OHV[NH3] = 11 9.99E-03 = B5-D4/B8+B8 12 1.00E-08 = B9*B10/B11 %3D 13 Kb - [NH4*][OH]/V[NH3] = 1.76E-05= D3-B12 2. LO