Consider two acids: HCO2H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO;H, pK = 5.UJ. (a) Which acid has the larger K? (b) Which acid is the stronger acid? (c) Which acid forms the stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the equilibrium lie further to the right?
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.
![Consider two acids: HCO2H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO,H, pK = 5.0].
(a) Which acid has the larger K? (b) Which acid is the stronger acid? (c) Which acid forms the
stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the
equilibrium lie further to the right?
%3D
The pKa values in Table 2.1 span a large range (-7 to 50). The pK, scale is logarithmic.
small difference in pK, translates into a large numerical difference, For example, the diffe
between the pK, of NH3 (38) and CH2=CH, (44) is six pKa units. This means that NH, is
one million times more acidic than CH,=CH,.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2512f01a-eeff-450f-9faa-ea73c2fb8250%2F34aedff6-452c-434b-98c4-237442008672%2Fqfi45fz_processed.jpeg&w=3840&q=75)
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