A student standardized her I 2 solution by preparing a solution of 0.0450 g of a

Question

A student standardized her I2 solution by preparing a solution of 0.0450 g of ascorbic acid (vitamin C) in a 100 mL volumetric flask. She titrated several 10.00 mL samples of the Vitamin C solution and found an average of 24.95 mL of I2 solution was required to get to the end point. Given that 25.0 mL of juice required an average of 15.1 mL of I2 solution to get to the end point, calculate the mass of vitamin C (ascorbic acid) in the juice sample.<?xml:namespace prefix = o ns = "urn:schemas-microsoft-com:office:office" />

Explanation / Answer

From my previous ans we have the molarity of the I2 solution:1.024*10^(-3)(M). now, the juice has molarity:(15.1/25)*1.024*10^(-3)(M)=6.184*10^(-4)(M).now,the mass of vitamin c in the juice sample:(25*6.184*10^(-4)*1000*176.12) gm= 2.722810^(-3)gm

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