Question

The net-ionic equation for an acid base reaction involves transfer of a proton (H ion) from the acid to the base. The products represent the conjugate base and acid of the reacting acid and base. The net-ionic equation for this system is shown here. HF-CN= F-HCN If you compare two acids and one is stronger than the other, how do the strengths of their conjugate bases compare? It is given that HF is the stronger acid. Which is the stronger base? the conjugate base of the stronger acid is the stronger base the conjugate base of the weaker acid is the stronger base Submit If the products of an acid-base reaction include a weaker acid and a weaker base than those in the reactants, does the reaction system favor formation of those products? yes Ono

Answer 1

Answer:

1. the conjugate base of the weaker acid is the stronger base is correct option

Since, we know from Lewis concept that, a stronger acid will have weaker conjugate base and weaker the acid have strong the conjugate base.

2. No, weak acid + weak base reaction , system doesn't favor

In case of these , when weak acid reacts with weak base , the equillbria always favors the left hand side ,for e.g.

CH2COOH. + H2O <======> CH2COO- + H3O+

here ,weak acid , acetic acid reacts with water , and thus the equillbria always tend to be left-hand side of the equillbria.

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