An ecobotanist separates the components of a tropical barkextract by chromatography. She discovers a large proportion ofquinidine, a dextrorotatory isomer of quinine used for control of arrhythmic heartbeat. Quinidine has two basic nitrogens (K(b1)=4.0X10⁻⁶ and K(b2)=1.0X10⁻¹⁰). To measure theconcentration, she carries out a titration. Because of the low solubility of quinidine, she first protonates both nitrogens withexcess HCl and titrates the acidified solution with standardized base. A 33.85-mg sample of quinidine (M=324.41g/mol) isacidified with 6.55 mL of 0.150 MHCl.(a) How many milliliters of 0.0133 MNaOH are needed to titrate the excess HCl?(b) How many additional milliliters of titrant are needed to reach the first equivalence point of quinidine dihydrochloride?(c) What is the pH at the first equivalence point?
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.
An ecobotanist separates the components of a tropical barkextract by chromatography. She discovers a large proportion ofquinidine, a dextrorotatory isomer of quinine used for control of arrhythmic heartbeat. Quinidine has two basic nitrogens (K(b1)=4.0X10⁻⁶ and K(b2)=1.0X10⁻¹⁰). To measure theconcentration, she carries out a titration. Because of the low solubility of quinidine, she first protonates both nitrogens withexcess HCl and titrates the acidified solution with standardized base. A 33.85-mg sample of quinidine (M=324.41g/mol) isacidified with 6.55 mL of 0.150 MHCl.(a) How many milliliters of 0.0133 MNaOH are needed to titrate the excess HCl?(b) How many additional milliliters of titrant are needed to reach the first equivalence point of quinidine dihydrochloride?(c) What is the pH at the first equivalence point?
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