A 200.0 mL sample of 0.216 M strong acid is titrated with 0.170 M strong base. Determine the pH of the solution before the addition of any strong base.
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.
A 200.0 mL sample of 0.216 M strong acid is titrated with 0.170 M strong base. Determine the pH of the solution before the addition of any strong base.
Strong acid – It is defined as an acid completely dissociate in aqueous solution called as strong acid.It has large capacity to give protons (H+) in aqueous solutions.
e.g. HCl, H2SO4, HNO3, HBr, HClO4 , HI
Weak acid- an acid dissociate slowly into its ions in an aqueous solution to give H+ ions
e.g. acetic acid.
Strong base- a base dissociate immediately into its ions in an aqueous solution to give OH- ions.
e.g. Sodium hydroxide.
Weak base-a base dissociate slowly into its ions in an aqueous solution to give OH- ions.
e.g. Ammonium hydroxide
At equivalence point of titration following three conditions can be observed-
- Titration between strong acid and strong base results in neutral solution.
- Titration between strong acid and weak base results in acidic solution.
- Titration between weak acid and strong base results in basic solution.
Answer of given numerical:
Consider,
Strong acid HA dissociate as follows and ICE table is
Where,I=Initial concentration,
C=Change in concentration,
E =Concentration at equilibrium
So,
[H3O+] =0.216 M
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