A beaker contains a water solution of unknown monoprotic* acid (molar mass of the acid is known to be 72.8 g/mol). The solution can be neutralized by Ca(OH)2. If it took 46.8 mL of 0.04 M Ca(OH)2 solution to react with all of the acid in 17.9 g of the solution, what is the mass percent of the acid in the solution? Roud the result (in %) up to one decimal place

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Q: concentrated

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