Calculate the mass % of acetic acid in the vinegar in the previous exercise (question#1 above). Assume that the density of the vinegar is 1.01 g mL.
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.
1) Given : volume of vinegar solution used = 2.50 mL
concentration of NaOH = 0.0960 M
volume of NaOH required = 34.90 mL
The reaction between NaOH and acetic acid is given by
NaOH + CH3COOH -------> CH3COONa + H2O
From the above reaction we can say that 1 mole of NaOH is required to neutralise 1 mole of CH3COOH and reach equivalence point.
Hence moles of NaOH required = moles of CH3COOH present
Since moles = concentration X volume of solution
=> concentration of acetic acid X volume of vinegar solution = concentration of NaOH X volume of NaOH solution
Hence substituting the values we get
concentration of acetic acid X 2.50 = 0.0960 X 34.90
=> concentration of acetic acid = 1.34 M approx
Given : 500 mL of vinegar solution = 0.5 L (since 1 L = 1000 mL)
Since moles = concentration X volume of solution in L
=> moles of acetic acid = 1.34 X 0.5 = 0.67 mol
Since molar mass of acetic acid =
Since mass = moles X molar mass
-> mass of acetic acid in 500 mL vinegar = 0.67 X 60 = 40.2 g
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