0.50 M solutions of each weak acid in the table are available. Choose an acid solution and determine what volume, in mL, of a 1.00 M NaOH solution should be added to 1.00 L of the acid solution to create a buffer with pH = 6.88. acid/base pairs to use: Ka pKa HCO2H/NaHCO2 1.8×10-4 3.74 H2CO3/NaHCO3 4.2×10-7 6.38 HBO3/NaH2BO3 7.3×10-10 9.14 NaHCO3/Na2CO3 4.8×10-11 10.32 HCO2H/NaHCO2 H2CO3/NaHCO3 H3BO3/NaH2BO3 NaHCO3/Na2CO3 ---------mL 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.
0.50 M solutions of each weak acid in the table are available. Choose an acid solution and determine what volume, in mL, of a 1.00 M NaOH solution should be added to 1.00 L of the acid solution to create a buffer with pH = 6.88.
| acid/base pairs to use: | Ka | pKa |
|---|---|---|
| HCO2H/NaHCO2 | 1.8×10-4 | 3.74 |
| H2CO3/NaHCO3 | 4.2×10-7 | 6.38 |
| HBO3/NaH2BO3 | 7.3×10-10 | 9.14 |
| NaHCO3/Na2CO3 | 4.8×10-11 | 10.32 |
---------mL NaOH
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