Question

в. pH Measurement Data 1. Sodium Acetate Solution O.lo m pH 8-73 pOH 5.2 [H,O]1.86xla (OH5.3l6 Using your experimental data, construct an ICE table, then calculate the equilibrium con- stant and the pK for the ion undergoing hydrolysis. Identify the equilibrium constant as either K, or K Experimental к. PK Calculate the actual value of the equilibrium constant using K and the K, reference value for acetic acid: K, 1.8 x 10s РК K_ Reference Calculate the % error using the pK values.

Answer 1

Ansi Sodium acetate icetate salt is salt a salt of strong base and weak acid so acetate ion undergo hydrolysis. CH₃COO + H₂O = CH₃COOH + OH - Req=kg = hydrolysis = kw constant for experimental result: [CH₂ Cco ] = 0 IM CH₃cco + H₂O² CH₃COOH + OH- to 0.14 - 0 0 t-teq 0.1(1-6) oth oth h-degree of hydrolysis, Cuien [OH-] = 5.37x10-6 1.0.1h05.378 10-6 kg = [CH₃COh] [ot] [Criz con ] ky [on]² [criz com] = [ok] = 0.1h 0.1(1h) kn = [on]² - [06]2 [04] = 0.16 011-oth 0.1-104] Green Com] = 5,37810-6 kn = (5 37x10 -6² 6:1-5:37x106) Kh = 2,88% 101 0.09999 lk : 2.88 X10-10 9.0 pk = -log(K) = -log (2.88810-10

For reference value Hydrolysis constant - Equilibrium constant - kw awen ka = 1,8x10-5 kw - 10-14 Ka keq = Kg = 10-14 118810-5 IK = 5.55 X 10 - 10 pk = -logk - = -log (5.55x10 to) [ pk = 9, 259 Yerror = 1 pkreference - pk experimental x 10 1 pkeeference 19.259-9.54) xico T 9,259 Xerror = 3.03%