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 Bronsted-Lowry Bronsted-Lowry acid neither base Br (aq) + H₂O (aq) HBr(aq) + H2O(l) HBr(aq) + H₂O() - - HBr(aq) + H2O(l) Br¯(aq) + H₂O' (aq) → Br¯ (aq) + H3O+ (aq) + Br (aq) + H2O (aq) - → HBr(aq) + H2O(l) О × о о о D

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 Bronsted-Lowry Bronsted-Lowry acid neither base Br (aq) + H₂O (aq) HBr(aq) + H2O(l) HBr(aq) + H₂O() - - HBr(aq) + H2O(l) Br¯(aq) + H₂O' (aq) → Br¯ (aq) + H3O+ (aq) + Br (aq) + H2O (aq) - → HBr(aq) + H2O(l) О × о о о D

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.7EP: Indicate whether the first listed reactant in each of the following BrnstedLowry acidbase reactions...

See similar textbooks

Similar questions

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
Ethanol (ethyl alcohol), CH3CH2OH, can act as a BrnstedLowry acid. Write the chemical equation for the reaction of ethanol as an acid with hydroxide ion, OH. Ethanol can also react as a BrnstedLowry base. Write the chemical equation for the reaction of ethanol as a base with hydronium ion, H3O+. Explain how you arrived at these chemical equations. Both of these reactions can also be considered Lewis acid base reactions. Explain this.
Classify each of the following statements as true or false: aAll Brnsted-Lowry acids are Arrhenius acids. bAll Arrhenius bases are Brnsted-Lowry bases, but not all Brnsted-Lowry bases are Arrhenius bases. c HCO3 is capable of being amphoteric. d HS is the conjugate base of S2. eIf the species on the right side of an ionization equilibrium are present in greater abundance than those on the left, the equilibrium is favored in the forward direction. f NH4+ cannot act as a Lewis base. gWeak bases have a weak attraction for protons. hThe stronger acid and the stronger base are always on the same side of a proton transfer reaction equation. iA proton transfer reaction is always favored in the direction that yields the stronger acid. jA solution with pH=9 is more acidic than one with pH=4. kA solution with pH=3 is twice as acidic as one with pH=6. lA pOH of 4.65 expresses the hydroxide ion concentration of a solution in three significant figures.
Indicate whether the first listed reactant in each of the following BrnstedLowry acidbase reactions is functioning as an acid or a base. a. HF + H2O H3O+ + F b. CN + H2O HCN + OH c. HCN + NO2 HNO2 + CN d. NH3 + HNO3 NH4+ + NO3
Indicate whether the first listed reactant in each of the following BrnstedLowry acidbase reactions is functioning as an acid or a base. a. F + H2O HF + OH b. HClO + H2O H3O+ + ClO c. H3PO4 + NH3 NH4+ + H2PO4 d. HNO2 + HS H2S + NO2
Pure liquid ammonia ionizes in a manner similar to that of water. (a) Write the equilibrium for the autoionization of liquid ammonia. (b) Identify the conjugate acid form and the base form of the solvent. (c) Is NaNH2 an acid or a base in this solvent? (d) Is ammonium bromide an acid or a base in this solvent?
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
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) HNO3+H2OH3O++NO3 (b) CN+H2OHCN+OH (c) H2SO4+CIHCI+HSO4 (d) HSO4+OHSO42+H2O (e) O2+H2O2OH (f) [Cu( H 2 O)3(OH)]++[Al( H 2 O)6]3+[Cu( H 2 O)4]2++[Al( H 2 O)5(OH)]2+ (g) H2S+NH2HS+NH3
8-13 Define (a) an Arrhenius acid and (b) an Arrhenius base.
Indicate whether or not the two members of each of the following pairs of substances constitute a conjugate acidbase pair. a. HCl and Cl b. NH4+ and NH3 c. H2CO3 and CO32 d. H2PO4 and HPO42
Natural gas frequently contains hydrogen sulfide, H2S. H2S is removed from natural gas by passing it through aqueous ethanolamine, HOCH2CH2NH2 (an ammonia derivative), which reacts with the hydrogen sulfide. Write the equation for the reaction. Identify each reactant as either a Lewis acid or a Lewis base. Explain how you arrived at your answer.
Boron trifluoride, BF3, and diethyl ether, (C2H5)2O, react to produce a compound with the formula BF3 : (C2H5)2O. A coordinate covalent bond is formed between the boron atom on BF3 and the oxygen atom on (C2H5)2O. Write the equation for this reaction, using Lewis electron-dot formulas. Label the Lewis acid and the Lewis base. Determine how many grams of BF3: (C2H5)2O are formed when 9.10 g BF3 and 23.3 g (C2H5)2O are placed in a reaction vessel, assuming that the reaction goes to completion.