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Na2S2O2 will crystallize out of solution when temperature is dropped down to 5 OC. A water solution that contains 2% soluble impurity and 50% Na2S2O2 . The solubility of the crystals are 1.5 lb/lb of free water. The soluble impurity also attaches to the crystals at a ratio of 0.7 lb solution/lb crystals. The final dry product of crystals must not contain more than 0.1% impurity. To ensure the impurity does not exceed this amount, how much water must be added to the solution before the temperature is dropped if the initial solution weighed 500 kg? How much Na2S2O2 will be generated in this process?

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