Hoping for solutions since I’m having a hard time with this. Pls skip if unsure or not willing to answer the subitems (these are all connected for one item). Thanks in advanced. Kriel just discovered a new protein, Krielase and for it not to unfold and lose its function, he realized that the protein needs to be constantly immersed in a pH = 6.50 solution. He is therefore interested in preparing a 50 mL 0.08 M pH = 4.50 buffer to contain the protein. He listed down the pure acids available to his disposal, and also looked for their acid dissociation constant (Ka) values. Acid Name Ka1 Ka2 Ka3 Nitrous Acid (HNO2) 4.00 x 10-4 N/A N/A Acetic Acid (CH3COOH) 1.76 x 10-5 N/A N/A Ascorbic Acid (HAsc) 7.90 x 10-5 1.60 x 10-12 N/A Phosphoric Acid (H3PO4) 7.52 x 10-3 6.23 x 10-8 4.28 x 10-13 A. Identify which weak acid system is best to use in preparing the buffer? Why? B. Identify the species which will make up the buffer system? Identify which one will neutralize the acidic disturbance, and the one which will react with an added base. C. Calculate the amount (in mmoles) of each of the components necessary to prepare the buffer? D. Indicate how Kriel is supposed to prepare the buffer from 6.0 M of the acid and 6.0 M NaOH.
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Hoping for solutions since I’m having a hard time with this. Pls skip if unsure or not willing to answer the subitems (these are all connected for one item). Thanks in advanced.
Kriel just discovered a new protein, Krielase and for it not to unfold and lose its function, he realized that the protein needs to be constantly immersed in a pH = 6.50 solution. He is therefore interested in preparing a 50 mL 0.08 M pH = 4.50 buffer to contain the protein. He listed down the pure acids available to his disposal, and also looked for their acid dissociation constant (Ka) values.
| Acid Name | Ka1 | Ka2 | Ka3 |
| Nitrous Acid (HNO2) | 4.00 x 10-4 | N/A | N/A |
| Acetic Acid (CH3COOH) | 1.76 x 10-5 | N/A | N/A |
| Ascorbic Acid (HAsc) | 7.90 x 10-5 | 1.60 x 10-12 | N/A |
| Phosphoric Acid (H3PO4) | 7.52 x 10-3 | 6.23 x 10-8 | 4.28 x 10-13 |
A. Identify which weak acid system is best to use in preparing the buffer? Why?
B. Identify the species which will make up the buffer system? Identify which one will neutralize the acidic disturbance, and the one which will react with an added base.
C. Calculate the amount (in mmoles) of each of the components necessary to prepare the buffer?
D. Indicate how Kriel is supposed to prepare the buffer from 6.0 M of the acid and 6.0 M NaOH.
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