Consider the titration of 40.0 mL of 0.0600 M (CH3)2NH (a weak base; Kb = 0.000540) with...

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Chemistry

Consider the titration of 40.0 mL of 0.0600 M(CH₃)₂NH (a weak base; K_b =0.000540) with 0.100 M HClO₄. Calculate the pH after thefollowing volumes of titrant have been added:

(a) 0.0 mL

pH =Â Â

(b) 6.0 mL

pH =Â Â

(c) 12.0 mL

pH =Â Â

(d) 18.0 mL

pH =Â Â

(e) 24.0 mL

pH =Â Â

(f) 26.4 mL

pH =Â Â

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3.7 Ratings (452 Votes)

a CH32NH H2O CH32NH 2 OH Kb 0000540 Kb OHCH32NH2CH32NH 0000540 XX 00600 X OH 00600000540 569103 pOH log OH 224 pH 14pOH1400224 1176 b 60 mL of 0100 M HClO4 added 60 mL 0100 M HClO4 adds 00006 mol of acid or H Here the original CH32NH solution See Answer

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(a) 0.0 mL pH =Â Â	(b) 6.0 mL pH =Â Â	(c) 12.0 mL pH =Â Â
(d) 18.0 mL pH =Â Â	(e) 24.0 mL pH =Â Â	(f) 26.4 mL pH =Â Â