Formic acid, HCO2H, is a weak acid (pKa = 3.74). Which of the following bases is sufficiently strong to deprotonate formic acid to an extent greater than 50% (25oC)? (pKb for each base is given) CH3CO2 - (9.24) IO3 - (13.2) ClCH3CO2 - (11.1) Reminder: pKa + pKb = 14.00 (25oC) Select one: A. ClCH3CO2 - only B. CH3CO2 - only C. IO3 - and ClCH3CO2 - D. IO3 - only
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.
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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.
Formic acid, HCO2H, is a weak acid (pKa = 3.74). Which of the following bases is sufficiently strong to deprotonate formic acid to an extent greater than 50% (25oC)? (pKb for each base is given)
CH3CO2 - (9.24) IO3 - (13.2) ClCH3CO2 - (11.1)
Reminder: pKa + pKb = 14.00 (25oC)
ClCH3CO2 - only
CH3CO2 - only
IO3 - and ClCH3CO2 -
IO3 - only
To deprotonate formic acid, base should be stronger than the conjugate base of formic acid. Stronger base would have lower value of pKb .
So first we would calculate pKb of conjugate base of formic acid and compare with pKb of given bases.
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