Which statement CORRECTLY explains the following acid-base reaction at equilibrium?
CH3H2C:- + HOC(CH3)3 <---> CH3CH3 + -:Ö:C(CH3)3
A. Weaker acid, HOC(CH3)3, and weaker base, CH3H2C:-, will be present in abundance.
B. Stronger acid, HOC(CH3)3, and stronger base, CH3H2C:-, will be present in abundance.
C. Weaker acid, CH3CH3, and stronger base, -:Ö:C(CH3)3, will be present in abundance.
D. Stronger acid, CH3CH3, and weaker base, -:Ö:C(CH3)3, will be present in abundance.
E. Weaker acid, CH3CH3, and weaker base, -:Ö:C(CH3)3, will be present in abundance
explanation:
Correct Answer: E
By nature, weak acids and weak bases are weakly dissociated to their respective conjugate bases and conjugate acids. Equilibrium position staying far right will only begin shifting to the left when stronger acids or stronger bases are added to the solution to selectively deplete CH3H2C:- or HOC(CH3)3 respectively. {Note: Reaction in the question involves an organometallic compound (Grignard Reagent); and it generally makes sense to consider the strong base, -:Ö:C(CH3)3, a weaker one when compared to CH3H2C:-}
I tried to understand the blue part but I just don't get it, so equilibrium shifts from right to left when you add strong acid, but if you're adding them to CH3H2C:- or HOC(CH3)3 to deplete them then the equilibrium should shift to the right (not left as they say) , am I correct??
please help