Asked by Mandy
In the titration of total acid with sodium hydroxide, NaOH, it was determined that 36.03mL of 0.0980M NaOH was needed to neutralize all the acid in a 10.0mL aliquot of a powdered drink mix solution. In a second titration, it was determined that were 1.45 x 10^(-5) moles of ascorbic acid in a 10.0mL aliquot of the same powdered drink mix solution. Calculate the moles of citric acid in the 10.0mL aliquot of powdered drink mix solution.
So confused.. Thank you.
So confused.. Thank you.
Answers
Answered by
DrBob222
I believe ascorbic acid is a diprotic acid which I will label as H2A.
Total mols NaOH used = M x L = approx 0.00353 mols NaOH.
The solution contained 1.45E-5 mols ascorbic and that will use 2*1.45E-5 = 2.90E-5 mols NaOH.
That leaves 0.003531-2.90E-5 = 0.00350 for mols NaOH to titrate the citric acid in the 10.0 mL sample. Since citric acid is a triprotic acid, mols citric acid will be 1/3 mols NaOH = 0.00350/3 = ?
Check my work.
Total mols NaOH used = M x L = approx 0.00353 mols NaOH.
The solution contained 1.45E-5 mols ascorbic and that will use 2*1.45E-5 = 2.90E-5 mols NaOH.
That leaves 0.003531-2.90E-5 = 0.00350 for mols NaOH to titrate the citric acid in the 10.0 mL sample. Since citric acid is a triprotic acid, mols citric acid will be 1/3 mols NaOH = 0.00350/3 = ?
Check my work.
Answered by
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If you had to make a pitcher of punch with a powdered drink mix, explain how this lab would allow making this drink in the least amount of time
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