14.50a | What is the effect on the concentrations of NO2−, HNO2, and OH− when HCl is added to a

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14.50b | What is the effect on the concentrations of NO2−, HNO2, and OH− when HNO2 is added to a 14.50b | What is the effect on the concentrations of NO2−, HNO2, and OH− when HNO2 is added to a
14.10a | How to identify the conjugate acid-base pairs in NO2− + H2O → HNO2 + OH− 14.10a | How to identify the conjugate acid-base pairs in NO2− + H2O → HNO2 + OH−
14.5b | Determine Ka for hydrogen sulfate ion, HSO4 −. In a 0.10-M solution the acid is 29% ionized. 14.5b | Determine Ka for hydrogen sulfate ion, HSO4 −. In a 0.10-M solution the acid is 29% ionized.
14.16 | The ionization constant for water (Kw) is 2.9 × 10^−14 at 40 °C. Calculate [H3O+], [OH−], pH 14.16 | The ionization constant for water (Kw) is 2.9 × 10^−14 at 40 °C. Calculate [H3O+], [OH−], pH
14.53b | How to calculate the Kb for ClO− from equilibrium concentrations 14.53b | How to calculate the Kb for ClO− from equilibrium concentrations
14.17 | The ionization constant for water (Kw) is 9.311 × 10^−14 at 60 °C. Calculate [H3O+], [OH−] 14.17 | The ionization constant for water (Kw) is 9.311 × 10^−14 at 60 °C. Calculate [H3O+], [OH−]
14.54a | How to calculate the Kb for NH3 from equilibrium concentrations 14.54a | How to calculate the Kb for NH3 from equilibrium concentrations
14.76a-b | The ion HTe− is an amphiprotic species; it can act as either an acid or a base. (a) What 14.76a-b | The ion HTe− is an amphiprotic species; it can act as either an acid or a base. (a) What