HClO4 M. a. Write the balanced reaction which occurs during the titration: Reaction: b. Label the diagram of a titration experiment. What solution is in the burette? What solution is in the beaker? 5 0 4 0 3 0 2 0 1 0 0 pH c. Determine the pH of the solution before the titration begins. pH =
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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 is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Consider the titration of 50.0 mL 0.1250 M KOH with 0.07500 HClO4 M.
a. Write the balanced reaction which occurs during the titration:
Reaction:
b. Label the diagram of a titration experiment. What solution is in the burette? What solution is in the beaker?
5
0
4
0
3
0
2
0
1
0
0
pH
c. Determine the pH of the solution before the titration begins. pH =
Under each species in the equation, classify as a strong acid (SA), strong base (SB), weak acid (WA) or a weak base (WB) or neutral (N).
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d. Determine the pH of the solution after the addition of 40.0mL acid. pH = ___________
e. Determine the pH of the solution at the equivalence point. pH = ___________
e. Determine the pH of the solution after 125.0mL acid has been added. pH = ___________
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