A chemist attempts to prepare some very pure crystals of borax
(sodium tetraborate, Na2B4O7 · 10 H2O) by dissolving 100 g of Na2B4O7 in 200 g of boiling water. He then carefully cools the solution slowly until some Na2B4O7 · 10 H2O crystallizes out. Calculate the grams of Na2B4O7 · 10 H2O recovered in the crystals per 100 g of total initial solution (Na2B4O7 plus H2O), if the residual solution at 55°C after the crystals are removed contains 12.4% Na2B4O7.
Hint: Treat the hydrated crystals as a separate stream leaving the process.
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