The following Ka values have been experimentally determined for formic and acetic acids. Acid Ka Formic acid, HCO2H 1.8x10-4 Acetic acid, CH3CO2H 1.8x10-5 Which of the following solutions will have the highest pH? 1.0 M sodium acetate, NaCH3CO2 1.0 M sodium formate, NaHCO2 1.0 M formic acid, HCO2H 1.0 M acetic acid, CH3CO2H Cannot be determined from the information given. What is the pH of a buffer solution
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.
| Acid | Ka |
| Formic acid, HCO2H | 1.8x10-4 |
| Acetic acid, CH3CO2H | 1.8x10-5 |
| 1.0 M sodium acetate, NaCH3CO2 |
| 1.0 M sodium formate, NaHCO2 |
| 1.0 M formic acid, HCO2H |
| 1.0 M acetic acid, CH3CO2H |
| Cannot be determined from the information given. |
What is the pH of a buffer solution of 0.10 M solution of acetic acid and 0.10 M sodium acetate? Support your answer.
For what pH is a formic acid/formate buffer best suited? Explain your answer.
Predict the magnitude (K >1, K<1, K = 1) for the equilibrium constant for the following reaction. Provide reasoning for your prediction.
HCOOH(aq) + CH3COO-(aq) <=> HCOO-(aq) + CH3COOH(aq)
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