Question

What is the pH of a solution containing 0.50 M ammonia and 0.50 M ammonium chloride? What will the pH be after 25mL of 0.20 M of hydrochloric acid has been added to 100.0mL of the solution containing the ammonia and ammonium chloride? What will the pH be after 18mL of 0.25 M of lithium hydroxide has been added to 100.0mL of the solution containing the ammonia and ammonium chloride? The ionization constant for ammonia is 1.8x10^-5.

Answer 1

@ NH3 | Nity formo a basse buffer POH= pkb (NH3) + loa [nity t] < conjugate world I og Ints ] < base = 4.75 + log 005070-50 = 4075 - pH = 14-POH = 14-4075 = 9.25 o Molarity of added (25 m2) x ( 0020M) tee =- crooro+25) mL = 0: 04 M NH3 + Hoel > Nituee Concentration deereares concentration proreases. New concentration of NH2 = 10.50-0.84 M = 0.46M u o ÑHe = (0.50 +0.04) M = 0.54M - pOH = 4.75 + log 0_54/0046 -[PHL = 14-4584 = 9.18

fing) Malarity of added LPOH = (18 ro1_) 60.25M). 1. (10000+ 18) mL = 0.038 M Nitz-H + L+ oH > Nity + H2O + pt concentration decreases concentration prereares New concentration of NH4 = (0150-01038) M = 0-462M " u u ( h = (0-50 + 6+ 68\M = 0 53% - pOH = 4.75 + log 01462/0538 = 4068 -PH= 14-4068 = 9.31

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