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I expected trimethylamine to be more basic than dimethylamine due to the increased $+I$ effect in trimethylamine. However in aqueous solution dimethylamine is more basic according to my textbook. Can someone please explain how? Is it because of hydrogen bonding?

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    $\begingroup$ You might want to look at the steric effects. The proton is 'less available' in $\ce{NMe3}$ than in $\ce{NHMe2}$, and so the molecule is less basic. $\endgroup$
    – Sonder
    Commented Sep 10 at 18:34
  • $\begingroup$ chemistry.stackexchange.com/questions/44560/… $\endgroup$
    – Mithoron
    Commented Sep 10 at 18:42

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