Experiment No: 3Determination of Ka, Kb, and % Ionization from pHName:Date:Experiment No: 3Objective: The purpose of this experiment is to learn determination of acid dissociationconstant (K a ) and of base dissociation constant (K b ) . In addition, the purpose is to learnpercent dissociation that is a measurement of the extent of ionization (%) .Results & Calculations:pH of tap water =6.24pH of de-ionized water =6.84pH of outgassed water with bubbles=4.53Solution01234567Molarity of6.0M1.2M0.24M0.048M0.0096M0.00192M0.00038M0.000768M1.502.102.552.893.183.273.443.600.170.380.861.924.299.5921.5515.16Ka of acetic acid02.8 10 55.26 10 53.31 10 53.46 10 54.55 10 51.50 10 43.347 10 48.22 10 5Calculated pH1.982.342.693.043.393.744.093.93HC 2 H 3O2ExperimentalpH% Dissociation=x 100MTakingk a = 1.76 10 5Acetic acid is a weak acid which partially dissociates in water to produce H 3 O + ion andthe conjugate base CH 3 COO The initial concentration of acetic acid is M 0CH 3COOH + H 2 O CH 3COO + H 3O +M0 xxxUsing the given value of K a and the equilibrium concentrations from the table, we haveExperiment No: 3x2= 1.76 10 5(M 0 x )x M 0 1.76 10 5 = 4.1952 10 3 M 0log (M 0 )1pH = log H 3O + = 3 log (4.1952) log ...
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