Each of the following acid-base reactions involves substances found in Table 1.8, Use the pKa data in the table to help you predict the products of the reactions. Use curved arrows to show electron flow. Predict whether the equilibrium lies to the left or to the right and calculate the equilibrium constant for each reaction. (a) HCCH+NH2 (b) HCCH+O2CH3 (c) (d) (e) TABLE 1.8 Acidity Constants (pKa) of Acids -For acid base reactions in which water is the solvent, the pKa of H3O+is zero and the pKa of H2O is 14 . Web collections of pKa data include that of H. Reich (University of Wisconsin) at httpsi/www.chem. wiscedu/areas/reichpkatable/ -For acid base reactions in which water is the solvent, the pKa of H3O+is zero and the pKa of H2O is 14 . The Bronsted-Lowry approach involving conjugate relationships between acids and bases makes a separate basicity constant Kb unnecessary. Rather than having separate tables listing Ka for acids and Kb for bases, the usual practice is to give only Ka or pKa as was done in Table 1.8. Assessing relative basicities requires only that we remember that the weaker the acid, the stronger the conjugate base and find the appropriate acid-base pair in the table