Experiment 1 Measurements Trial #1 Trial #2 volume of NaOH dispensed in the titration at the color change (mL) Determined Molarity of NaOH (mol/L) mass of benzoic acid used (g) pH of benzoic acid solution before titration initial volume reading on the burette before titration 0.0 mL 0.0 mL (mL) 0.244 g 0.244 g 2.97 2.97 Trial #1 0.244 2.97 0.0 mL volume reading on the burette at the color change 20.0 mL 20.0 mL 20.0 mL (mL) 20.0 mL 20.0 mL 20.0 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.
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.
Experiment 1. Find the Molarity of NaOH (mol/L) for each trial. Then calculate the average Molarity. See attached table.
Experiment 2. Find the Molarity of the unknown solution using the titration data in the experiment 2 table and using the average molarity of NaOH calculated in Experiment#1. See attached table.
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