The ability of a solution to resist changes to the pH from added acid or base depends upon the amount of weak acid and weak base. The buffering capacity is the ratio of weak acid to weak base and the best buffering occurs when these are equal, making the buffering capacity equal to 1. In the above buffer the buffering capacity is the ratio of [H2PO4-1] to [HPO4-2], or Ka [H2PO4-1] Ka (4.44 x 10-5) Ka (8) [H3O+1] = ––––––––––––– = –––––––––––––––– = ––––––––– [HPO4-2] (5.55 x 10-5) (10) Here the buffering capacity is close to 1 (0.8) and so the buffering capacity is Blank 1. Fill in the blank, read surrounding text. When the buffering capacity is 1, the [H3O+1] = Ka and the pH = pKa This helps chemists choose the right buffer for the needed pH. To buffer at pH = 7, the weak acid should a pKa of close to 7, True or False ? Blank 2. Fill in the blank, read surrounding text. the weak acid should have Ka of close to 1 x 10-7, True or False ? Blank 3. Fill in the blank, read surrounding text.
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.
The ability of a solution to resist changes to the pH from added acid or base depends upon the amount of weak acid and weak base. The buffering capacity is the ratio of weak acid to weak base and the best buffering occurs when these are equal, making the buffering capacity equal to 1. In the above buffer the buffering capacity is the ratio of
[H2PO4-1] to [HPO4-2], or
Ka [H2PO4-1] Ka (4.44 x 10-5) Ka (8)
[H3O+1] = ––––––––––––– = –––––––––––––––– = –––––––––
[HPO4-2] (5.55 x 10-5) (10)
Here the buffering capacity is close to 1 (0.8) and so the buffering capacity is Blank 1. Fill in the blank, read surrounding text.
When the buffering capacity is 1, the [H3O+1] = Ka
and the pH = pKa
This helps chemists choose the right buffer for the needed pH. To buffer at pH = 7,
the weak acid should a pKa of close to 7, True or False ? Blank 2. Fill in the blank, read surrounding text.
the weak acid should have Ka of close to 1 x 10-7, True or False ? Blank 3. Fill in the blank, read surrounding text.
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