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.
![(We breathe out CO2 gas. In our blood CO, is present as carbonic acid which has a pka of 6.36.)
donating one proton to water to produce bicarbonate anio
(e)
(b)
2. Protons transfer immediately between acids and bases to reach an equilibrium. In the following
acid base reactions, draw Lewis structures for the conjugate acid and conjugate base formed when the
reactants (on the left) are mixed.
(a) CH;C(=0)0H + NH3
acetic acid
Acid
(conj, acid
(conj, base)
(b) HC(=0)0H
formic acd
+ CH3CH2NH2
(conj. acid
(conj. base)
(c) CH CH,CH2C(=0)OH + Na/OH (Na'/CrJ + H2O +
butanoic acid
3. By definition the pH of a dilute solution of a weak acid equals its pKa only when the concentrations of
unionized acid [HA] equals the concentration of its ionized conjugate base [A1. At any given pH an acid will be
mostly ionized or unionized depending on its pKa. Given the following weak acids and their pka's decide
whether the acid is mostly ionized or mostly unionized at the pH shown.
la] CHC=0)OH [pKa = 4:76] at pH = 5.76
[b] HC(=0)OH [pKa 3.75]
at pH = 2.75
[c] CH.CH,CH,NH, [pKa = 10.7] at pH = 8.7
fd H,S
[pka = 7.0]
at pH = 2
le] CH,OH
IpKa = 15.5] at pH= 9.5](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1eb89e89-76b2-4183-a288-e599bf80b5f6%2F229fb8a3-9ebb-4e63-b18c-40c90a29ed85%2Ff5xa9r_processed.jpeg&w=3840&q=75)
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