Consider the titration of 70.0 mL of 0.0300 M (CH3)3N (a weak
base; Kb = 6.40e-05)...
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Chemistry
Consider the titration of 70.0 mL of 0.0300 M (CH3)3N (a weakbase; Kb = 6.40e-05) with 0.100 M HBr. Calculate the pH after thefollowing volumes of titrant have been added:
(a) 0.0 mL
pH = _____
(b) 5.3 mL
pH = _____
(c) 10.5 mL
pH = _____
(d) 15.8 mL
pH = _____
(e) 21.0 mL
pH = _____
(f) 27.3 mL
pH = _____
Answer & Explanation
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4.5 Ratings (796 Votes)
aThe initial pHconsider the reactionYou need to do and ICE table to calculate the disociation ofthe baseInitial003M00ChangeXXXEquilibrium003XXXUsing the mass action equationand the concentrations at equilibriumSolving for X you will get the concentrationsusingthe quadratic formulabYou added a strong acid thus all the H willl react toneutralize the
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