Calculating Vitamin C Content in Orange Juice using Titration Method

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SUMMARY

The forum discussion focuses on calculating the Vitamin C content in orange juice using the titration method. The user provided a titration setup with a 20.00 mL orange juice sample diluted to 170 mL with deionised water, utilizing a standard iodine solution of 0.005 mol L-1 and 26.2 mL of iodine. The proposed equation for calculating the concentration of ascorbic acid was critiqued, emphasizing the need for stoichiometry and correct use of concentrations rather than mass. Key resources for further understanding stoichiometry and dilution in titration were also shared.

PREREQUISITES
  • Understanding of titration techniques and procedures
  • Knowledge of stoichiometry in chemical reactions
  • Familiarity with molarity and concentration calculations
  • Basic chemistry concepts, including reaction equations
NEXT STEPS
  • Learn about stoichiometric calculations in titration
  • Study the principles of dilution and concentration
  • Explore the use of molar mass in chemical calculations
  • Review resources on titration calculations and methodologies
USEFUL FOR

Chemistry students, laboratory technicians, and anyone involved in quantitative analysis of vitamin content in food and beverages.

jstretto

Homework Statement


Titration:
Volume of orange juice: 20.00 mL
Final diluted volume: orange juice + 150mL of deionised water: 170 mL
Standard Iodine solution concentration: 0.005 mol L-1
Amount of Iodine used: 26.2mL

Homework Equations


Is this equation right?

(Concentration of Iodine Solution * Volume of Iodine used) * (Diluted Volume/Volume of orange juice) * Mass of ascorbic acid * 1000 to get from g/100mL to mg/100mL

The Attempt at a Solution



(0.005*0.0262)*(170/20)*176.12*1000
[/B]
196.10962

I feel like there might be something wrong with the equation I am using. Any help would be greatly appreciated
 
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Instead of using an "equation" why don't you try to just follow stoichiometry and dilution? That's the only sure method of doing every titration problem, no matter if you were given some equation to use, or not.

Start by writing the reaction equation.
 
You need to use concentration of Ascorbic Acid rather than mass, as you cannot mix up grammes and mols.
You also need an equals sign.
And you may need a factor like 2 or 3 somewhere which you will find from the chemical reaction formula. For instance,
H2SO4 + 2 NaOH = 2NaSO4 + 2H2O.
 
tech99 said:
You need to use concentration of Ascorbic Acid rather than mass

You are missing the point of the formula. Description is lousy, but the formula as given makes logical sense, especially taking into account fact the number used by OP (176.12) is a molar mass.

And you may need a factor like 2 or 3 somewhere which you will find from the chemical reaction formula.

Not exactly, there is also another factor that has to be taken into account, as the answer must be given per 100 mL.
 
I am quite new to this all, do you have any links/keywords I could google to try follow stochiometery and dilution.

I've got the reaction equation

C6H8O6 +I2 -> 2I- + C6H6O6
 
Thank you so much
 

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