For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither. reaction highlighted reactant acid Bronsted-Lowry Bronsted-Lowry base neither I (aq) + H2O(l) → HI(aq) + OH¯(aq) 0 Ο HI(aq) + OH (aq) → I (aq) + H₂O(l) O I (aq) + H2O(l) 1 HI(aq) + OH (aq) O HI(aq) + OH(aq) I (aq) + H2O(l) - O O

Write chemical equations that show the indicated behavior in aqueous solution for each of the following chemical species. a. HOCl behaves as a BrnstedLowry acid b. NH3 behaves as a BrnstedLowry base c. H2PO4 behaves as a BrnstedLowry acid d. CO32 behaves as a BrnstedLowry base

In the following net ionic reaction, identify each species as either a Brnsted-Lowry acid or a Brnsted -Lowry base: CH3COO(aq)+HS(aq)CH3COOH(aq)+S2(aq). Identify the conjugate of each reactant and state whether it is a conjugate acid or a conjugate base.

Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ion

Identify and label the Bronsted-Lowry acid, its conjugate base, the Bronsted-Lowry base, and its conjugate acid in each of the following equations: (a) NO2+H2OHNO2+OH (b) HBR+H2OH3O++Br (c) HS-+H2OH2S+OH (d) H2PO4+OHHPO42+H2O (e) H2PO4+HClH3PO4+Cl (f) [Fe( H 2 O)5(OH)]2++[Al( H 2 O)6]3+[Fe( H 2 O)6]3++[Al( H 2 O)5(OH)]2+ (g) CH3OH+HCH3O+H2

12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’

Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.

In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) C2H5N(aq) + CH3CO2H(aq) C5H5NH+(aq) + CH3CO2(aq) (b) N2H4(aq) + HSO4(aq) N2H5+(aq) + SO42(aq) (c) [Al(H2O)6]3+ (aq) + OH(aq) [Al(H2O)5OH]2+ (aq) + H2O+()

Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?

Without writing an equation, specify the molecular ratio in which each of the following acidbase pairs will react. a. HCl and KOH b. H2CO3 and KOH c. HCl and Ca(OH)2 d. H2CO3 and Ca(OH)2