For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither. highlighted reactant reaction Bronsted-Lowry Bronsted-Lowry neither acid base I (aq) + H2O(l) HI(aq) + OH (aq) о о I (aq) + H2O(l) HI(aq) + OH (aq) O о о HI(aq) + OH (aq). - I 1 (4) + НО(0) O O HI(aq) + OH (aq) - -> (ад) + Н20(1) о о O X

For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither. highlighted reactant reaction Bronsted-Lowry Bronsted-Lowry neither acid base I (aq) + H2O(l) HI(aq) + OH (aq) о о I (aq) + H2O(l) HI(aq) + OH (aq) O о о HI(aq) + OH (aq). - I 1 (4) + НО(0) O O HI(aq) + OH (aq) - -> (ад) + Н20(1) о о O X

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter17: Acid-base(proton Transfer) Reactions

Section: Chapter Questions

Problem 12E

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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.
. In each of the following chemical equations, identify the conjugate acid-base pairs. a. NH3(aq)+H2O(l)NH4+(aq)+OH(aq) b. PO43(aq)+H2O(1)HPO42(aq)+OH(aq) c. C2H3O2(aq)+H2O(l)HC2H3O2(aq)+OH(aq)
5. Given the general equation illustrating the reaction of the acid HA in water, HA(aq)+H2O(l)H3O+(aq)+A(aq)explain why water is considered a base in the Brønsted-Lowry model.
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
Calculate the pKa value for each of the following acids. a. Nitrous acid (HNO2), Ka = 4.5 104 b. Carbonic acid (H2CO3), Ka = 4.3 107 c. Dihydrogen phosphate ion (H2PO4), Ka = 6.2 108 d. Sulfurous acid (H2SO3), Ka = 1.5 102
. a. Write the conjugate acid for each of the following Brønsted-Lowry bases. NO3.HSO4,ClO4,NH3,HCO3b. Write the conjugate base for each of the following Brønsted- Lowry acids. HCI,H2SO4,NH3,NH4,HCO3
The sec-butyl cation can react as both a Brnsted-Lowry acid (a proton donor) and a Lewis acid (an electron pair acceptor) in the presence of a watersulfuric acid mixture. In each case, however, the product is different. The two reactions are as follows: (a) In which reaction(s) does this cation react as a Lewis acid? In which reaction(s) does it react as a Brnsted-Lowry acid? (b) Write Lewis structures for reactants and products and show by the use of curved arrows how each reaction occurs.
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’
The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107
The pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.
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+()