$$ \ce{HX(aq) + Y-(aq) <--> HY(aq) + X-(aq)} \hskip{2em} K_{eq} \gt 1 $$

A solution of a salt of a weak acid \(\ce{HY}\) is added to a solution of another weak acid \(\ce{HX}\). Based on the information given above, which of the following species is the strongest base?

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Since \(K_{eq}\gt 1\), the products are favored. This must mean that the reaction between the reactants goes closer to completion than the reverse reaction. This implies that \(\ce{Y-}\) does a good job of drawing \(\ce{H+}\) from the acid. The ability to draw protons corresponds to the Brønsted-Lowry definition of a base.