Experiment 4 - pH=2.81[H]=1.549*10-3 M[NaOH]=5.10*10-2 M...

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Experiment 4: Determination of Acid Constant, K a DATA/ RESULTS Table 1- Data and Calculation for Standardization Trials Mass(g) Volume(ml) [NaOH] M 1 0.5030 g 26.71 ml 9.17*10 -2 M 2 0.5006 g 26.65 ml 9.19*10 -2 M 3 0.5006 g 26.73 ml 9.165*10 -2 M Average Concentration of NaOH= 9.175*10 -2 M KHP mass=204.22g, molar ratio between KHP and NaOH is 1:1 Table 2- Titration Data (Part II) for Acetic Acid/K a from Equilibrium Expression . (Unknown # C) Trials Volume (ml) Mol of NaOH (mol) 1 31.35 ml 2.878*10 -3 mol 2 31.52 ml 2.892*10 -3 mol 3 31.43 ml 2.88*10 -3 mol Average: 31.43 ml 2.88*10 -3 mol molar ratio between KHP and NaOH is 1:1
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Unformatted text preview: pH=2.81, [H + ]=1.549*10-3 M [NaOH]=5.10*10-2 M Ka=(1.549*10-3 )/((5.10*10-2 )-(1.549*10-3 )) =4.85*10-5 Table 3- Titration Data from Part III(Titration Curves) (Unknown # C) Intial reading pH of acetic acid: pH2.93 [H + ]=0.00175 trials Equivalent pH Half-Equivalent pH Volume at euilvalent (ml) Molarity (mol/ L) pK a K a 1 9.63 4.45 29.571ml 0.04972 4.563 0.00002735 2 9.91 4.38 35.111ml 0.05359 Avg 9.77 4.415 32.341ml 0.05165 Comparison of the acetic acid solution molarities and Ka’s...
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This note was uploaded on 03/08/2011 for the course CHEM 102 taught by Professor Duzut during the Spring '11 term at Los Angeles City College.

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