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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 Solved by verified expert
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    See Answer
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