Microorganisms are grown in laboratory bioreactors to study their effectiveness in destroying hazardous organic compounds. Ammonium...

  

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Microorganisms are grown in laboratory bioreactors to study their effectiveness in destroying hazardous organic compounds. Ammonium chloride (NH,CI) is a soluble salt that is often added to the reactor to provide a source of the nutrient nitrogen to the microorganisms. Consider a 2 L closed vessel that is half filled with otherwise pure water. A quantity of 500 mg of ammonium chloride is completely dissolved in the water. Some of the ammonium ions (NH4+) dissociate to form ammonia (NH3) and liberate a proton (H+). Some of the ammonia molecules escape into the gas phase. (a) Set up a system of equations that you could use to solve for the equilibrium pH of the water. (b) Calculate the equilibrium pH. You may do this either by using some chemistry intuition (though you must justify your simplifying assumptions!) or by solving the system of equations (using your calculator or Maple or Excel or whatever equation solver of your choice). Potentially useful DATA: Temperature Henry's constant for NH3 at 20°C Acid dissociation constant for NH4* 20 °C KH = 62 M atm-¹ PKA = 9.23 Microorganisms are grown in laboratory bioreactors to study their effectiveness in destroying hazardous organic compounds. Ammonium chloride (NH4Cl) is a soluble salt that is often added to the reactor to provide a source of the nutrient nitrogen to the microorganisms. Consider a 2 L closed vessel that is half filled with otherwise pure water. A quantity of 500 mg of ammonium chloride is completely dissolved in the water. Some of the ammonium ions (NH,+) dissociate to form ammonia (NH3) and liberate a proton (H+). Some of the ammonia molecules escape into the gas phase. (a) Set up a system of equations that you could use to solve for the equilibrium pH of the water. (b) Calculate the equilibrium pH. You may do this either by using some chemistry intuition (though you must justify your simplifying assumptions!) or by solving the system of equations (using your calculator or Maple or Excel or whatever equation solver of your choice). Potentially useful DATA: Temperature Henry's constant for NH3 at 20°C Acid dissociation constant for NH4* 20 °C KH 62 M atm-¹ PKA = 9.23 Microorganisms are grown in laboratory bioreactors to study their effectiveness in destroying hazardous organic compounds. Ammonium chloride (NH4CI) is a soluble salt that is often added to the reactor to provide a source of the nutrient nitrogen to the microorganisms. Consider a 2 L closed vessel that is half filled with otherwise pure water. A quantity of 500 mg of ammonium chloride is completely dissolved in the water. Some of the ammonium ions (NH4+) dissociate to form ammonia (NH3) and liberate a proton (H+). Some of the ammonia molecules escape into the gas phase. (a) Set up a system of equations that you could use to solve for the equilibrium pH of the water. (b) Calculate the equilibrium pH. You may do this either by using some chemistry intuition (though you must justify your simplifying assumptions!) or by solving the system of equations (using your calculator or Maple or Excel or whatever equation solver of your choice). Potentially useful DATA: Temperature Henry's constant for NH3 at 20°C Acid dissociation constant for NH4* 20 °C KH 62 M atm-¹ PKA = 9.23 Microorganisms are grown in laboratory bioreactors to study their effectiveness in destroying hazardous organic compounds. Ammonium chloride (NH,CI) is a soluble salt that is often added to the reactor to provide a source of the nutrient nitrogen to the microorganisms. Consider a 2 L closed vessel that is half filled with otherwise pure water. A quantity of 500 mg of ammonium chloride is completely dissolved in the water. Some of the ammonium ions (NH4+) dissociate to form ammonia (NH3) and liberate a proton (H+). Some of the ammonia molecules escape into the gas phase. (a) Set up a system of equations that you could use to solve for the equilibrium pH of the water. (b) Calculate the equilibrium pH. You may do this either by using some chemistry intuition (though you must justify your simplifying assumptions!) or by solving the system of equations (using your calculator or Maple or Excel or whatever equation solver of your choice). Potentially useful DATA: Temperature Henry's constant for NH3 at 20°C Acid dissociation constant for NH4* 20 °C KH = 62 M atm-¹ PKA = 9.23 Microorganisms are grown in laboratory bioreactors to study their effectiveness in destroying hazardous organic compounds. Ammonium chloride (NH4Cl) is a soluble salt that is often added to the reactor to provide a source of the nutrient nitrogen to the microorganisms. Consider a 2 L closed vessel that is half filled with otherwise pure water. A quantity of 500 mg of ammonium chloride is completely dissolved in the water. Some of the ammonium ions (NH,+) dissociate to form ammonia (NH3) and liberate a proton (H+). Some of the ammonia molecules escape into the gas phase. (a) Set up a system of equations that you could use to solve for the equilibrium pH of the water. (b) Calculate the equilibrium pH. You may do this either by using some chemistry intuition (though you must justify your simplifying assumptions!) or by solving the system of equations (using your calculator or Maple or Excel or whatever equation solver of your choice). Potentially useful DATA: Temperature Henry's constant for NH3 at 20°C Acid dissociation constant for NH4* 20 °C KH 62 M atm-¹ PKA = 9.23 Microorganisms are grown in laboratory bioreactors to study their effectiveness in destroying hazardous organic compounds. Ammonium chloride (NH4CI) is a soluble salt that is often added to the reactor to provide a source of the nutrient nitrogen to the microorganisms. Consider a 2 L closed vessel that is half filled with otherwise pure water. A quantity of 500 mg of ammonium chloride is completely dissolved in the water. Some of the ammonium ions (NH4+) dissociate to form ammonia (NH3) and liberate a proton (H+). Some of the ammonia molecules escape into the gas phase. (a) Set up a system of equations that you could use to solve for the equilibrium pH of the water. (b) Calculate the equilibrium pH. You may do this either by using some chemistry intuition (though you must justify your simplifying assumptions!) or by solving the system of equations (using your calculator or Maple or Excel or whatever equation solver of your choice). Potentially useful DATA: Temperature Henry's constant for NH3 at 20°C Acid dissociation constant for NH4* 20 °C KH 62 M atm-¹ PKA = 9.23

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To calculate the equilibrium pH of the water in the bioreactor when 500 mg of ammonium chloride NH4Cl is dissolved in it we need to consider the disso... View the full answer