Final answer:
The farther the equilibrium position lies toward the products, the stronger the reactants originally used in the acid-base reaction. A higher equilibrium constant (K > 10^3) indicates a reaction favoring the formation of products, while a lower K (K < 10^-3) signifies a reaction that favors reactants.
Step-by-step explanation:
The equilibrium position of an acid-base reaction provides insight into the relative strengths of the acids and bases involved. When considering a reaction like H2O and CH2COOH, one can determine which is the stronger acid by looking at which direction the equilibrium lies. If the equilibrium lies far to the right (toward the products), it means the reactants were stronger acids and bases, because a strong acid and a strong base react to form a weaker acid and a weaker base, according to the Brønsted-Lowry definition. Therefore, in the context of the student's question: The farther the equilibrium position lies toward the products, the stronger the acid or base.
It is also essential to understand that the equilibrium constant (K) can indicate the tendency of a reaction. For example, a value of K > 103 generally indicates that the reaction has a strong tendency to form products. This is the case with the reaction between H2 and Cl2 to produce HCl, which essentially proceeds to completion. Conversely, a value of K < 10-3 signifies that the reaction favors the formation of reactants more than products.