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when comparing the basic nature of $CH_3O^-$ and that of $OH^-$. I found two arguments. one favoring the more basic nature of $CH_3O^-$ and the other favoring the basic nature of $OH^-$. so which of them is true. and why isn't the other condition correct.

the conditions are as follows.

  1. since $CH_3OH$ is a stronger acid when compared to $H_2O$, its corresponding conjugate base should be weaker. that is $CH_3O^-$ is a weaker base when compared to $OH^-$
  2. since there exists a methyl group on the $O^-$ the electron density on $O^-$ increases hence it is a better base when compared to $OH^-$ since H doesn't have any +I effect /
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  • $\begingroup$ Point 1) seems out of nothing $\endgroup$ – Alchimista Oct 24 at 9:11
  • $\begingroup$ What makes you think CH3OH is a stronger acid than H2O ? $\endgroup$ – Poutnik Oct 24 at 9:17
  • $\begingroup$ Their pKa values $\endgroup$ – Rohit Raj Oct 25 at 6:10

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