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Question

The amount of lactic acid, HC3H5O3, produced in a sample of muscle tissue was analysed by reaction with hydroxide ion. Hydroxide ion was produced in the sample mixture by electrolysis. The cathode reaction was,
2H2O(l)+2eH2(g)+2OH(aq.)
Hydroxide ion reacts with lactic acid as soon as it is produced. The end point of the reaction is detected with an acid-base indicator. It required 115 seconds for a current of 15.6 mA to reach end point. How many grams of lactic acid (a monoprotic acid) were present in the sample?

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Solution

No. of moles of lactic acid = No. of mole of OH used
= No. of faraday used in electrolysis
Number of faraday used =I×t96500=15.6×103×11596500
=1.86×105
Mass of lactic acid = Number of moles × Molecular mass
=1.86×105×90=1.674×103g.

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