ACID-BASE TITRATION Link: You tube: Acid Base Titration (Vinegar Titration) SMARTERTEACHER ANALYSIS OF VINEGAR: Vinegar

[answerhappygod]

ACID-BASE TITRATION Link: You tube: Acid Base Titration (Vinegar
Titration) SMARTERTEACHER ANALYSIS OF VINEGAR: Vinegar is a dilute
solution of acetic acid. Law requires that vinegar should be at
least 4% acetic acid by weight. Measure exactly 5ml of vinegar into
an 250ml Erlenmeyer flask. Add 25ml of water and 4 to 5 drops of
phenolphthalein indicator. Titrate with the standard solution
(0.1N) sodium hydroxide. Need to reach a point, where the whole
solution stays very light pink for 1 min or so. Close the stopcock
and note down the volume inside the buret. Do not overrun the end
point. Calculation: The volume of sodium hydroxide times its
normality equals the number of milligram equivalents of acetic acid
neutralized. The equivalent of acetic acid is 60.0mg or 0.060g. The
5ml sample of vinegar weighs 5.05g. Example of Calculation: 24 ml
vol of NaOH (what was left in the buret when you reached the end
point in the flask) X 0.1N=2.4mlequivX60mg (the equivalent of
acetic acid is 60mg) =144mg 144mg/ 5.O25g(5ml of vinegar=5.025g)
X100 = % 1. What is meant by standard solution? 2. Define:
Molarity; Normality 3. What are the glass wares used in the vinegar
titration? 4. What are the solutions used in the vinegar titration?
5. What is the function of the phenolphthalein used in this
titration? 6. If one overruns the end point, what can be done to
correct it? 7. In titrating, why is it necessary to be sure that
the stopcock is held in place? 8. Calculations: VOLUME OF
STANDARDIZED BASE (in the buret) ________________42.3ml PERCENTAGE
OF ACETIC ACID_______________________________ % • SHOW CALCULATIONS
HERE (step by step):