Concentration Using Titration
Determining the percent Concentration of a given Solution using Titration
Morphy Kuffour
Mrs. Langlis, AP Chemistry C-D
9/24/2017
Purpose:
Determining the precise concentration of vinegar through titration using a standard solution of Potassium Hydroxide (KOH) (aq)
Background:
Vinegar is a solution of acetic acid (CH3COOH) in water. The concentration of acetic acid in
Vinegar is written as a Molarity (mol/L). In this experiment, titration is used to determine the concentration of acetic acid in vinegar. Titration is an experimental technique for determining the concentration of a solution by reaction with something else. To perform a titration, a carefully measure amount of one reactant is added to an Erlenmeyer flask. An indicator is added …show more content…
Using a clean plastic weighing dish, obtain between 1.50 g of potassium hydrogen phthalate ( C8H5KO4) to a 125 Erlenmeyer flask and add about 50 mL of water. Swirl the flask to dissolve the KHP. Record the exact mass of KHP that you use.
6. Transfer all of the KHP to a very clean Erlenmeyer flask along with approximately 50 ml of deionized water. Squirt some …show more content…
Swirl the flask.
7. Add two of phenolphthalein indicator to the flask and swirl to mix.
Safety:
Goggles must worn including Lab coats and gloves can be worn if need be or when it’s appropriate. KOH is corrosive. If KOH solution splashes into your eyes or comes contact with skin, use the eyewash or flush the affected area with water.
Waste Disposal:
All solutions can be flushed down the sink with plenty of water.
Data and Calculations:
Table 1: Titration of KOH and KHP
Run Initial (mL) Final (mL) Equivalence Point (mL)
Rough 3.0 4.9 4.6
1 4.9 9.0 4.1
2 9.0 12.0 4
3 12.0 16.1 4.1
Average value for Equivalence point (mL) 4.2
Table 2: Vinegar Titration: 10.00 ml vinegar used for each titration
Run Initial (mL) Final (mL) Equivalence Point (mL)
Rough .2 5.4 5.2
1 5.4 10.7 5.3
2 20.4 25.5 5.1
3 25.5 30.7 5.2
Average value for Equivalence point (mL) 5.2
Conclusion:
In this experiment, an unknown concentration of unknown weak acid (acetic acid) was analyzed. We mad three trials, and the average molarity of the vinegar was determined to be 0.868 M. I found the percentage of the acetic acid, HC2H3O2(aq), in the vinegar to be
Morphy Kuffour
Mrs. Langlis, AP Chemistry C-D
9/24/2017
Purpose:
Determining the precise concentration of vinegar through titration using a standard solution of Potassium Hydroxide (KOH) (aq)
Background:
Vinegar is a solution of acetic acid (CH3COOH) in water. The concentration of acetic acid in
Vinegar is written as a Molarity (mol/L). In this experiment, titration is used to determine the concentration of acetic acid in vinegar. Titration is an experimental technique for determining the concentration of a solution by reaction with something else. To perform a titration, a carefully measure amount of one reactant is added to an Erlenmeyer flask. An indicator is added …show more content…
Using a clean plastic weighing dish, obtain between 1.50 g of potassium hydrogen phthalate ( C8H5KO4) to a 125 Erlenmeyer flask and add about 50 mL of water. Swirl the flask to dissolve the KHP. Record the exact mass of KHP that you use.
6. Transfer all of the KHP to a very clean Erlenmeyer flask along with approximately 50 ml of deionized water. Squirt some …show more content…
Swirl the flask.
7. Add two of phenolphthalein indicator to the flask and swirl to mix.
Safety:
Goggles must worn including Lab coats and gloves can be worn if need be or when it’s appropriate. KOH is corrosive. If KOH solution splashes into your eyes or comes contact with skin, use the eyewash or flush the affected area with water.
Waste Disposal:
All solutions can be flushed down the sink with plenty of water.
Data and Calculations:
Table 1: Titration of KOH and KHP
Run Initial (mL) Final (mL) Equivalence Point (mL)
Rough 3.0 4.9 4.6
1 4.9 9.0 4.1
2 9.0 12.0 4
3 12.0 16.1 4.1
Average value for Equivalence point (mL) 4.2
Table 2: Vinegar Titration: 10.00 ml vinegar used for each titration
Run Initial (mL) Final (mL) Equivalence Point (mL)
Rough .2 5.4 5.2
1 5.4 10.7 5.3
2 20.4 25.5 5.1
3 25.5 30.7 5.2
Average value for Equivalence point (mL) 5.2
Conclusion:
In this experiment, an unknown concentration of unknown weak acid (acetic acid) was analyzed. We mad three trials, and the average molarity of the vinegar was determined to be 0.868 M. I found the percentage of the acetic acid, HC2H3O2(aq), in the vinegar to be