Buttercup acid is an organic compound that is a liquid at room temperature and is neutralized by strong bases: C4H8O2(aq) + OH-(aq) ----> C4H7O2-(aq) + H2O(I). Compute the volume of a 0.150 M aqueous solution of NaOH that would be necessary to neutralize 0.215 g of butyric acid.
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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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.
Buttercup acid is an organic compound that is a liquid at room temperature and is neutralized by strong bases: C4H8O2(aq) + OH-(aq) ----> C4H7O2-(aq) + H2O(I). Compute the volume of a 0.150 M aqueous solution of NaOH that would be necessary to neutralize 0.215 g of butyric acid.
Given : Mass of butyric acid = 0.215 g
Concentration of NaOH solution = 0.150 M
The reaction taking place is
=> C4H8O2 (aq) + NaOH (aq) ---------> C4H7O2Na (aq) + H2O (l)
Molar mass of C4H8O2 = Atomic mass of C X 4 + Atomic mass of H X 8 + Atomic mass of O X 2 = 12 X 4 + 1 X 8 + 16 X 2 = 88 g/mol
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