CHEM103 Study Guide - Final Guide: Lewis Structure, Valence Electron, Ionic Bonding

Acids that ionize extensively in solution are referred to as a. dissociators. b. weak electrolytes. c. Arrhenius acids d. Bronsted-Lowry acids. e. strong acids. According to the Bronsted-Lowry definition, a base a. increases the H_3O^+ concentration in an aqueous solution. b. increases the OH^- concentration in an aqueous solution. c. is a proton acceptor. d. is a proton donor. e. is an electron-pair donor. In the following reaction HCO^-_3(aq) + H_2O(I) rightarrow CO^2-_3(aq) + H_3O^+(aq) a. HCO^-_3 is an acid and H_2O is its conjugate base. b. HCO^-_3 is an acid and CO^2-_3 is its conjugate base. c. H_3O^+ is an acid and HCO^-_3 is its conjugate base. d. H_2O is an acid and CO^2-_3 is its conjugate base. e. H_3O^+ is an acid and CO^2-_3 is its conjugate base. The conjugate acid of HSO^-_ is _____ a. OH^- b. SO^2-_4 c. H_2SO_4 d. H_2O e. H_3O^+ What is the H_3O^+ concentration of an aqueous solution with a pH of 12.17? a. 6.8 times 10^-13 M b. 1.9 times 10^-9 M c. 5.2 times 10^-6 M d. 1.5 times 10^-2 M e. 1.1 M What is the OH^- concentration of an aqueous solution with a pH of 11.45? (K_w = 1.0 times 10^-4) a. 3.5 times 10^-12 M b. 9.4 times 10^-10 M c. 1.1 times 10^-5 M d. 2.8 times 10^-3 M e. 7.8 times 10^-2 M An aqueous solution with a pH of 3.00 is diluted from 2.0 L to 4.0 L. What is the pH of the diluted solution? a. 1.50 b. 1.73 c. 3.00 d. 3.30 e. 6.00