Calculating Vitamin C Content in Orange Juice using Titration Method

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Discussion Overview

The discussion revolves around calculating the vitamin C content in orange juice using the titration method. Participants are addressing the appropriate equations and stoichiometric principles necessary for accurate calculations in a chemistry homework context.

Discussion Character

  • Homework-related
  • Technical explanation
  • Mathematical reasoning

Main Points Raised

  • One participant presents a calculation method involving the concentration of iodine solution, volume used, and mass of ascorbic acid, but expresses uncertainty about the correctness of the equation.
  • Another participant suggests focusing on stoichiometry and dilution rather than relying solely on a formula, emphasizing the importance of writing the reaction equation.
  • Several participants indicate that concentration of ascorbic acid should be used instead of mass, and that an equals sign is necessary in the equation.
  • There is mention of needing a factor from the chemical reaction formula, with examples provided, but the exact factor required remains unspecified.
  • A participant shares the balanced reaction equation for ascorbic acid and iodine, indicating progress in understanding the stoichiometry involved.
  • Links to external resources for further understanding of stoichiometry and dilution are provided by participants.

Areas of Agreement / Disagreement

Participants generally agree on the need to use concentration rather than mass and the importance of stoichiometry in titration calculations. However, there is no consensus on the specific equation to use or the factors required in the calculations, leaving the discussion unresolved.

Contextual Notes

Participants have not fully resolved the mathematical steps involved in the calculations, and there are references to factors that depend on the specific chemical reaction, which have not been clarified.

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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