the c-h bond in acetone, (ch3)2c=o, has a pka of 19.2. draw two resonance structures for its conjugate base. then, explain why acetone is much more acidic than propane, ch3ch2ch3 (pka = 50).
Added by Julian C.
Step 1
Step 1:** Draw the resonance structures for the conjugate base of acetone, (CH3)2C=O, after losing a proton: \[ \text{Structure 1: } \chemfig{CH_3-C(=[::+60]O)-CH_2^{-}} \] \[ \text{Structure 2: } \chemfig{CH_3-C(=O^{-})-CH_3} \] ** Show more…
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The $\mathrm{C}-\mathrm{H}$ bond in acetone, $\left(\mathrm{CH}_{3}\right)_{2} \mathrm{C}=\mathrm{O},$ has a $\mathrm{p} K_{\mathrm{a}}$ of $19.2 .$ Draw two resonance structures for its conjugate base. Then, explain why acetone is much more acidic than propane, $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}\left(\mathrm{p} K_{\mathrm{a}}=50\right)$
The $\mathrm{C}-\mathrm{H}$ bond in acetone, $\left(\mathrm{CH}_{3}\right)_{2} \mathrm{C}=\mathrm{O}$, has a $\mathrm{pK}_{\mathrm{a}}$ of $19.2 .$ Draw two resonance structures for its conjugate base. Then, explain why acetone is much more acidic than propane, $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}\left(\mathrm{pK}_{\mathrm{a}}=50\right)$.
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