16.78 (a) Given that K, for ammonia is 1.8 X 10-5 and that for hydroxylamine is 1.1 X 10-8, which is the stronger base? (b) Which is the stronger acid, the ammonium ion or the hydroxylammonium ion? (c) Calculate Ka values for NH 16.91 Indicate w false. For to make i and H3NOH*. creases fr 16.79 Using data from Appendix D, calculate [OH¯]and pH for each ble. (b) I of the following solutions: (a) 0.10 M NaBrO, (b) 0.080 M NaHS, (c) a mixture that is 0.10 M in NaNO2 and 0.20 M in Ca(NO2)2. Tcing data from Appendix D, calculate [OH ] and pH acid strer bonded a strong than S. for each of the following solutions: (a) 0.105 M NaF, (b) 0.035 M Na2S, (c) a mixture that is 0.045 M in 16.92 Indicat false. F NaCH3COO and 0.055 M in Ba(CH3COO)2. to mak 16.81 A solution of sodium acetate (NaCH3COO) has a pH of 9.70. What is the molarity of the solution? cules i same the ce 1682 Pyridinium bromide (C5H5NHB1) is a strong electrolyte that dissociates completely into C5H5NH* and Br¯. An aqueous solution of pyridinium bromide has a pH of 2.95. electr know elem (a) Write out the reaction that leads to this acidic pH. Lewis Ac (b) Using Appendix D, calculate the Ka for pyridinium bromide. 16.93 Amr bas (c) A solution of pyridinium bromide has a pH of 2.95. What is the concentration of the pyridinium cation at equilibrium, in units of molarity? 16,83 Predict whether aqueous solutions of the following com- pounds are acidic, basic, or neutral: (a) NHĄBr, (b) FeCl3, (C) Na2CO3, (d) KCIO4, (e) NaHC2O4. rea ert tio 16.94 Th (a 16.84 Predict whether aqueous solutions of the following sub- (b stances are acidic, basic, or neutral: (a) AlCl3, (b) NaBr, C) NACIO, (d) [CH3NH3]NO3, (e) Na,SO3. 16.85 An unknown salt is either NaF, NaCl, or NaOCl. When 0.050 O F00 Lof solution, APPENDIX AQUEOUS EQUILIBRIUM CONSTANTS TABLE D.1 Dissociation Constants for Acids at 25 °C Kat К.г. Каз Name Formula 1.8 x 10-5 CH,COOH (or HC,H,O2) 1.0 x 10-7 3.0 X 10-12 Acetic acid 5.6 x 10 3 Arsenic acid H3ASO4 5.1 x 10 10 Arsenous acid H3ASO3 1.6 X 10-12 8.0 X 10-5 Ascorbic acid H2C,H6O6 6.3 x 10-5 Benzoic acid C,H3COOH (or HC,HSO2) 5.8 x 10-10 Boric acid HзВОЗ 1.5 X 10 5 Butanoic acid C3H,COOH (or HC4H,O2) 5.6 X 10-11 4.3 x 10-7 Carbonic acid H2CO3 Chloroacetic acid 1.4 X 10-3 CH-CICOOH (ог НС2H2О2CI) Chlorous acid 1.1 X 10-2 A. HCIO2 7.4 X 10-4 1.7 x 10-5 4.0 X 10-7 Citric acid HOOCC(OH)(CH2COOH)2 (or H3C,H5O7) Cyanic acid 3.5 X 10-4 HCNO Formic acid НСООН (or НСНО2) 1.8 X 10-4 Hydroazoic acid HN3 1.9 x 10-5 Hydrocyanic acid HCN 4.9 X 10-10 Hydrofluoric acid HF 6.8 X 10-4 Hydrogen chromate ion HCГО4 3.0 x 10-7 Hydrogen peroxide НО2 2.4 X 10-12 Hydrogen selenate ion HSEO, 2.2 x 10-2 Hydrogen sulfide H2S 9.5 x 10-8 1 x 10-19 Hypobromous acid HBГО 2.5 x 10-9 Hypochlorous acid HCIO 3.0 x 10-8 Hypoiodous acid HIO 2.3 X 10-11 Iodic acid HIOЗ 1.7 X 10-1 Lactic acid CH,CH(ОН)СООН (or HC3H503) 1.4 X 10-4 Malonic acid CH2(COOH)2 (or H2C3H2O4) 1.5 x 10-3 2.0 x 10-6 1996 Nitrous acid HNO2 4.5 x 10-4 Oxalic acid (COOH)2 (or H2C2O4) Paraperiodic acid 5.9 x 10-2 6.4 X 10-5 H;IO6 Phenol 2.8 X 10-2 5.3 x 10-9 C,H5OH (or HC,H;O) Phosphoric acid 1.3 x 10-10 НаРОД Propionic acid 7.5 x 10-3 6.2 x 10-8 4.2 x 10-13 CH-СООН (or НСЗН,О2) Pyrophosphoric acid 1.3 x 10-5 НАР.О, Selenous acid 3.0 x 10-2 4.4 x 10-3 2.1 X 10 -7 H2SEO3 Sulfuric acid 2.3 x 10-3 5.3 x 10-9 H2SO4 Sulfurous acid H,SO3 Strong acid 1.2 X 10-2 Tartaric acid HОOC(CHOH),CООН (or H-C,Н,О) 1.7 X 10-2 6.4 X 10-8 1092 1.0 X 10-3

16.78 (a) Given that K, for ammonia is 1.8 X 10-5 and that for hydroxylamine is 1.1 X 10-8, which is the stronger base? (b) Which is the stronger acid, the ammonium ion or the hydroxylammonium ion? (c) Calculate Ka values for NH 16.91 Indicate w false. For to make i and H3NOH. creases fr 16.79 Using data from Appendix D, calculate [OH¯]and pH for each ble. (b) I of the following solutions: (a) 0.10 M NaBrO, (b) 0.080 M NaHS, (c) a mixture that is 0.10 M in NaNO2 and 0.20 M in Ca(NO2)2. Tcing data from Appendix D, calculate [OH ] and pH acid strer bonded a strong than S. for each of the following solutions: (a) 0.105 M NaF, (b) 0.035 M Na2S, (c) a mixture that is 0.045 M in 16.92 Indicat false. F NaCH3COO and 0.055 M in Ba(CH3COO)2. to mak 16.81 A solution of sodium acetate (NaCH3COO) has a pH of 9.70. What is the molarity of the solution? cules i same the ce 1682 Pyridinium bromide (C5H5NHB1) is a strong electrolyte that dissociates completely into C5H5NH and Br¯. An aqueous solution of pyridinium bromide has a pH of 2.95. electr know elem (a) Write out the reaction that leads to this acidic pH. Lewis Ac (b) Using Appendix D, calculate the Ka for pyridinium bromide. 16.93 Amr bas (c) A solution of pyridinium bromide has a pH of 2.95. What is the concentration of the pyridinium cation at equilibrium, in units of molarity? 16,83 Predict whether aqueous solutions of the following com- pounds are acidic, basic, or neutral: (a) NHĄBr, (b) FeCl3, (C) Na2CO3, (d) KCIO4, (e) NaHC2O4. rea ert tio 16.94 Th (a 16.84 Predict whether aqueous solutions of the following sub- (b stances are acidic, basic, or neutral: (a) AlCl3, (b) NaBr, C) NACIO, (d) [CH3NH3]NO3, (e) Na,SO3. 16.85 An unknown salt is either NaF, NaCl, or NaOCl. When 0.050 O F00 Lof solution, APPENDIX AQUEOUS EQUILIBRIUM CONSTANTS TABLE D.1 Dissociation Constants for Acids at 25 °C Kat К.г. Каз Name Formula 1.8 x 10-5 CH,COOH (or HC,H,O2) 1.0 x 10-7 3.0 X 10-12 Acetic acid 5.6 x 10 3 Arsenic acid H3ASO4 5.1 x 10 10 Arsenous acid H3ASO3 1.6 X 10-12 8.0 X 10-5 Ascorbic acid H2C,H6O6 6.3 x 10-5 Benzoic acid C,H3COOH (or HC,HSO2) 5.8 x 10-10 Boric acid HзВОЗ 1.5 X 10 5 Butanoic acid C3H,COOH (or HC4H,O2) 5.6 X 10-11 4.3 x 10-7 Carbonic acid H2CO3 Chloroacetic acid 1.4 X 10-3 CH-CICOOH (ог НС2H2О2CI) Chlorous acid 1.1 X 10-2 A. HCIO2 7.4 X 10-4 1.7 x 10-5 4.0 X 10-7 Citric acid HOOCC(OH)(CH2COOH)2 (or H3C,H5O7) Cyanic acid 3.5 X 10-4 HCNO Formic acid НСООН (or НСНО2) 1.8 X 10-4 Hydroazoic acid HN3 1.9 x 10-5 Hydrocyanic acid HCN 4.9 X 10-10 Hydrofluoric acid HF 6.8 X 10-4 Hydrogen chromate ion HCГО4 3.0 x 10-7 Hydrogen peroxide НО2 2.4 X 10-12 Hydrogen selenate ion HSEO, 2.2 x 10-2 Hydrogen sulfide H2S 9.5 x 10-8 1 x 10-19 Hypobromous acid HBГО 2.5 x 10-9 Hypochlorous acid HCIO 3.0 x 10-8 Hypoiodous acid HIO 2.3 X 10-11 Iodic acid HIOЗ 1.7 X 10-1 Lactic acid CH,CH(ОН)СООН (or HC3H503) 1.4 X 10-4 Malonic acid CH2(COOH)2 (or H2C3H2O4) 1.5 x 10-3 2.0 x 10-6 1996 Nitrous acid HNO2 4.5 x 10-4 Oxalic acid (COOH)2 (or H2C2O4) Paraperiodic acid 5.9 x 10-2 6.4 X 10-5 H;IO6 Phenol 2.8 X 10-2 5.3 x 10-9 C,H5OH (or HC,H;O) Phosphoric acid 1.3 x 10-10 НаРОД Propionic acid 7.5 x 10-3 6.2 x 10-8 4.2 x 10-13 CH-СООН (or НСЗН,О2) Pyrophosphoric acid 1.3 x 10-5 НАР.О, Selenous acid 3.0 x 10-2 4.4 x 10-3 2.1 X 10 -7 H2SEO3 Sulfuric acid 2.3 x 10-3 5.3 x 10-9 H2SO4 Sulfurous acid H,SO3 Strong acid 1.2 X 10-2 Tartaric acid HОOC(CHOH),CООН (or H-C,Н,О) 1.7 X 10-2 6.4 X 10-8 1092 1.0 X 10-3

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter15: Acids And Bases

Section: Chapter Questions

Problem 15.49QP

See similar textbooks