Anonymous
Anonymous asked in Science & MathematicsChemistry · 5 months ago

Commercial hydrochloric acid is 38 percent HCl by mass. The density is of this aqueous solution is 1.19g/cm^3?

What is the molarity of hydrochloric acid in this solution?

What mass of solution is required to give 796 milligrams of hydrochloric acid?

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  • 5 months ago
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    (1.19 g/cm^3) x (1000 cm^3 / 1 L) x (0.38) / (36.4611 g HCl/mol) = 12.4 mol/L HCl

    [I'm not convinced aqueous HCl exists in such a high concentration, but that's what the given numbers say.]

    (796 mg HCl) / (0.38) = 2095 mg solution

    • Roger the Mole
      Lv 7
      5 months agoReport

      https://www.sigmaaldrich.com/chemistry/stockroom-reagents/learning-center/technical-library/reagent-concentrations.html

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