Question
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to...
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 3.00 ✕ 102 mL of solution and then titrate the solution with 0.163 M NaOH.
C6H5CO2H(aq) + OH-(aq) 
C6H5CO2-(aq) + H2O(ℓ)
What are the concentrations of the following ions at the equivalence point?
Na+, H3O+, OH-
C6H5CO2-
M Na+
M H3O+
M OH-
M C6H5CO2-
What is the pH of the solution?
Answers
120 =0.00641M 1 mol 0.235 g X 70 Concentration of CH.COOH, (C,H,COOH) = -02007 Concentration of NaOH added=0.163 M ICE table: CH,COOH + OH - CH,COO + H, I(M): 0.00641 0.163 C(M): -0.00641 -0.00641 +0.00641 E(M): 0.08 0.157 0.00641 + According to the equilibrium table, [OH-] = (x) M = 0.157 M [CH.000- ] = (x) M = 0.157 M [CH,COOH ) = (0.00641-0.00641) M = 0 M According to ionic product of water, [H0]= 0.157 = 6.37x10-1 M pH = -log[H,0+1=-log(6.37x10-14) = 13.20 onic product of water, [H30*]= Ky = 1.0x10-14
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