Answer to Question #113587 in General Chemistry for Emma

Question

In the following equilibrium, predict whether the reactants or products will be favoured and explain by comparing the relative strengths of the acids involved in the Brönsted–Lowry acid–base reaction.


H2C6H5O7– + HSO3– -> H3C6H5O7 + SO32–

Answer 1

Solution:According to the Bronsted-Lowry theory, the acid – proton donor (Bronsted acid) and its conjugated base — any compound capable of attaching a proton (Bronsted base) — always take part in the chemical interaction of acids and bases. Since the base can be considered as a product of the removal of the proton from the acid, the electric charge of the conjugated acid is always one less than the charge of the base conjugated with it.

AH + B → BH⁺ + A^- ,

where AH is acid, B is base, BH + is acid coupled to B, and A is base coupled to AH.

H₂C₆H₅O₇ + HSO₃– -> H₃C₆H₅O₇ + SO₃^2–;

H₂C₆H₅O₇ - is base; HSO₃ is acid; H₃C₆H₅O₇-citric acid; SO₃²–is base coupled to HSO₃.

Answer: The reagents will react.