Home >
Community >
What is the enthalpy of neutralization of acetic acid and sodium bicarbonate?
Upvote
9
Downvote
+ Acetic acid
+ Sodium
+ Chemistry
+ Sodium bicarbonate
Posted by
Nicholas Williams
What is the enthalpy of neutralization of acetic acid and sodium bicarbonate?
Since acetic acid is a weak electrolyte, we will use its Ka for the remainder of our calculations. Using the Henderson-Hasselbach equation, pH=pKa+log([base]/[acid]). Inputting our information, 4=4.76+log([base]/[acid]). Therefore, the ratio of the concentration of Sodium Bicarbonate to that of acetic acid must be 10^(-0.76). Since there is no more information, I can only offer an example of a buffer system that would work. Suppose we have two solutions of acetic acid and sodium bicarbonate with equivalent molarities. The buffer must then have the ratio of the number of liters of Sodium Bicarbonate to the number of liters of Acetic acid equal to 10^(-0.76). So 100 mL of Sodium Bicarbonate in aqueous solution and 173.78 mL of Acetic acid in aqueous solution, assuming the two solutions have an equal concentration, will yield a buffer with a pH of 4.
Since acetic acid is a weak electrolyte, we will use its Ka for the remainder of our calculations. Using the Henderson-Hasselbach equation, pH=pKa+log([base]/[acid]). Inputting our information, 4=4.76+log([base]/[acid]). Therefore, the ratio of the concentration of Sodium Bicarbonate to that of acetic acid must be 10^(-0.76). Since there is no more information, I can only offer an example of a buffer system that would work. Suppose we have two solutions of acetic acid and sodium bicarbonate with equivalent molarities. The buffer must then have the ratio of the number of liters of Sodium Bicarbonate to the number of liters of Acetic acid equal to 10^(-0.76). So 100 mL of Sodium Bicarbonate in aqueous solution and 173.78 mL of Acetic acid in aqueous solution, assuming the two solutions have an equal concentration, will yield a buffer with a pH of 4.
For general information and equations about enthalpy, see the following website: https://chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Thermodynamics/State_Functions/Enthalpy/Standard_Enthalpy_Of_Formation . This is the best one I found on-line. For specific values for enthalpy of various chemicals, there is a table (as well a more definitions and equations about thermodynamics) in Chapter 5 of the CRC Handbook of Chemistry, by the Chemical Rubber Company, updated annually with lots and lots of information about chemical compounds. It's expensive, but a good university library should have it.
For general information and equations about enthalpy, see the following website: https://chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Thermodynamics/State_Functions/Enthalpy/Standard_Enthalpy_Of_Formation . This is the best one I found on-line. For specific values for enthalpy of various chemicals, there is a table (as well a more definitions and equations about thermodynamics) in Chapter 5 of the CRC Handbook of Chemistry, by the Chemical Rubber Company, updated annually with lots and lots of information about chemical compounds. It's expensive, but a good university library should have it.
Since acetic acid is a weak electrolyte, we will use its Ka for the remainder of our calculations. Using the Henderson-Hasselbach equation, pH=pKa+log([base]/[acid]). Inputting our information, 4=4.76+log([base]/[acid]). Therefore, the ratio of the concentration of Sodium Bicarbonate to that of acetic acid must be 10^(-0.76). Since there is no more information, I can only offer an example of a buffer system that would work. Suppose we have two solutions of acetic acid and sodium bicarbonate with equivalent molarities. The buffer must then have the ratio of the number of liters of Sodium Bicarbonate to the number of liters of Acetic acid equal to 10^(-0.76). So 100 mL of Sodium Bicarbonate in aqueous solution and 173.78 mL of Acetic acid in aqueous solution, assuming the two solutions have an equal concentration, will yield a buffer with a pH of 4.
Since acetic acid is a weak electrolyte, we will use its Ka for the remainder of our calculations. Using the Henderson-Hasselbach equation, pH=pKa+log([base]/[acid]). Inputting our information, 4=4.76+log([base]/[acid]). Therefore, the ratio of the concentration of Sodium Bicarbonate to that of acetic acid must be 10^(-0.76). Since there is no more information, I can only offer an example of a buffer system that would work. Suppose we have two solutions of acetic acid and sodium bicarbonate with equivalent molarities. The buffer must then have the ratio of the number of liters of Sodium Bicarbonate to the number of liters of Acetic acid equal to 10^(-0.76). So 100 mL of Sodium Bicarbonate in aqueous solution and 173.78 mL of Acetic acid in aqueous solution, assuming the two solutions have an equal concentration, will yield a buffer with a pH of 4.
More
VOTE
For general information and equations about enthalpy, see the following website:
https://chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Thermodynamics/State_Functions/Enthalpy/Standard_Enthalpy_Of_Formation . This is the best one I found on-line. For specific values for enthalpy of various chemicals, there is a table (as well a more definitions and equations about thermodynamics) in Chapter 5 of the CRC Handbook of Chemistry, by the Chemical Rubber Company, updated annually with lots and lots of information about chemical compounds. It's expensive, but a good university library should have it.
For general information and equations about enthalpy, see the following website:
https://chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Thermodynamics/State_Functions/Enthalpy/Standard_Enthalpy_Of_Formation . This is the best one I found on-line. For specific values for enthalpy of various chemicals, there is a table (as well a more definitions and equations about thermodynamics) in Chapter 5 of the CRC Handbook of Chemistry, by the Chemical Rubber Company, updated annually with lots and lots of information about chemical compounds. It's expensive, but a good university library should have it.
More
VOTE