Write the formulas for the conjugate acid of each of the following bases. a. H_2
ID: 529380 • Letter: W
Question
Write the formulas for the conjugate acid of each of the following bases. a. H_2O b. CO^2-_3 c. PH_3 Which of the following would you expect to act as Bronsted-Lowry bases: a) Br- b) Li+ c) H_3PO_4 d) NH^+_4 e) H_2O f) NH^-_2 For each of the following reactions, identify the Bronsted-Lowry acid and Bronsted-Lowry base on the reactant side of the equation, and the conjugate acid and conjugate base on the product side. a. HSO^-_4(aq) + CO^2-_3(aq) SO^2-_4(aq) HCO^-_3(aq) b. HCO^-_3(aq) + OH^-(aq) CO^2-_3(aq) + H_2O(l) Consider the following two reactions. In which reaction does H_2PO^-_4 act as a base? In which does it act as an acid? Is H_2PO^-_4 an acid or base? a. H_2PO^-_4(aq) + H_2O(l) H_3PO_4(aq) + OH^-(aq) b. H_2PO^-_4(aq) + H_2O(l) HPO^2-_4 (aq) + H_3O^-(aq)Explanation / Answer
7.Conjugate acid is obtained by adding H+ ion to the given base
(a) The conjugate acid of H2O is H2O + H+ ------> H3O+
(a) The conjugate acid of CO32- is CO3 2- + H+ ---> HCO3-
(a) The conjugate acid of PH3 is PH3 + H+ ----> PH4+
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