Acidity or Basicity of Salt Solutions. Will 0.10 M aqueous solutions of the following salts be acidic, basic or neutral? (Assume a solution is neutral if its pH is 7.00±0.05). Equilibrium constants may be found in an appendix to your text. ✰ ammonium sulfide ((NH4)2S) ✰ sodium hydrogen oxalate (NaHC204) ✰ ammonium formate (NH 4 CHO2) ✰ sodium sulfate (Na2SO4) ✰ sodium chloride (NaCl)

Acidity or Basicity of Salt Solutions. Will 0.10 M aqueous solutions of the following salts be acidic, basic or neutral? (Assume a solution is neutral if its pH is 7.00±0.05). Equilibrium constants may be found in an appendix to your text. ✰ ammonium sulfide ((NH4)2S) ✰ sodium hydrogen oxalate (NaHC204) ✰ ammonium formate (NH 4 CHO2) ✰ sodium sulfate (Na2SO4) ✰ sodium chloride (NaCl)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.80QE: Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus...

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Tartaric acid is a weak diprotic fruit acid with Ka1 = 1.0 103 and Ka2 = 4.6 105. a Letting the symbol H2A represent tartaric acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about 0.5 M in tartaric acid. c Calculate the pH of a 0 0250 M tartaric acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentration in solutions b and c?
Malic acid is a weak diprotic organic acid with Ka1 = 4.0 104 and Ka2 = 9.0 105. a Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about one molar in malic acid. c Calculate the pH of a 0.0175 M malic acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentrationin in solutions b and c?
Methylammonium chloride is a salt of methylamine, CH3NH2. A 0.10 M solution of this salt has a pH of 5.82. a Calculate the value for the equilibrium constant for the reaction CH3NH3++H2OCH3NH2+H3O+ b What is the Kb value for methylamine? c What is the pH of a solution in which 0.450 mol of solid methylammonium chloride is added to 1.00 L of a 0.250 M solution of methylamine? Assume no volume change.
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Ionization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.
Lactic acid, C3H6O3, occurs in sour milk as a result of the metabolism of certain bacteria. Calculate the pH of a solution of 56. mg lactic acid in 250. mL water. Ka for D-lactic acid is 1.5 × 10−4.
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Acidity or Basicity of Salt Solutions. Will 0.10 M aqueous solutions of the following salts be acidic, basic or neutral? (Assume a solution is neutral if its pH is 7.00±0.05). Equilibrium constants may be found in an appendix to your text. ammonium sulfide ((NH4)2S) ✓ammonium cyanide (NH4CN) ✓ammonium dihydrogen phosphate (NH4H₂PO4) ammonium acetate (NH4C₂H3O₂) ✓sodium fluoride (NAF)
Will 0.10 M aqueous solutions of the following salts be acidic, basic or neutral? (Assume a solution is neutral if its pH is 7.00±0.05). Equilibrium constants may be found in an appendix to your text. ammonium formate (NH4CHO₂) ammonium acetate (NH4C₂H302) sodium hydrogen arsenate (Na₂HASO4) sodium acetate (NaC₂H30₂) ammonium sulfide ((NH4)2S)