A titration can define the volume of one solution required to react correctly with an identified volume of a different solution. Titration commonly comprises of reactions such as redox reactions and reactions involving precipitations, different than acid-base reactions.
“Titration can discern the volume of one solution required to react exactly with a known volume of a different solution.”
The equation for Titration Formula is articulated as:
Where,
1000 = factor relating mg to grams
W = mass of sample
N = normality of titrant
V = volume of titrant
Eq.wt = equivalent weight of acid
Though commonly the Titration Formula is articulated as:
Where,
V1 = Volume of titrant
N = Normality of titrant
V2 = Volume of sample
Eq.wt = equivalent weight of predominant acid
Solved Examples
Problem 1: Compute the titratable acidity if 17.5ml of 0.085N NaOH is required to titrate a 15ml sample of juice, the sum titratable acidity of that juice, articulated as percent citric acid. (molecular weight = 192; equivalent weight = 64)
Solution:
Now we use the equation:
% of acid = 0.085×17.5×64/15×10 = 0.635%
Notice that the equivalent weight of anhydrous citric acid always is used in calculating and reporting the results of titration.
Problem 2: Contemplate the reaction of sulfuric acid H2SO4 with sodium hydroxide NaOH.
H2SO4 + 2NaOH à 2H2O + Na2SO4
How many millimeters of 0.250M NaOH must be added to react completely with the sulfuric acid? Assuming that a beaker contains 35.0mL of 0.175M H2SO4.
Answer:
The calculation is as follows.
= 4.90 ×× 10-2 L NaOH
precisely 49.0 mL of 0.250M sodium hydroxide solution reacts with 35.0 mL of 0.175M sulfuric acid solution.
