Consider the titration of 30.0 mL of 0.0700 M (CH3)3N (a weak base; Kb = 6.40e-05) with...

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Chemistry

Consider the titration of 30.0 mL of 0.0700 M(CH₃)₃N (a weak base; K_b =6.40e-05) with 0.100 M HCl. Calculate the pH after the followingvolumes 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) 39.9 mL

pH = ______

Answer & Explanation Solved by verified expert

4.0 Ratings (798 Votes)

For CH33N let us assume CH33N B for simplicity so CH33N H2O CH33NH OH becomes B H2O HB OH Kb HBOHB so a no volume of acid B H2O HB OH Kb HBOHB in equilibrium for 1 mol of OH we hava always 1 mol of HB HB OH x the dissociation fraction of acid B Mx 007x Account for dissociation 64105 xx007x solve with quadratic formula x OH 0002084 pOH logOh log0002084 268110 pH 14pOH 14268110 113189 b 53 mL See Answer

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(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) 39.9 mL pH = __________