What is the molarity of a 93% Nitric acid solution?
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OK, I understand that molarity is moles of solute/Litres of solution. With a high mass percentage of the HNO3 which is more then the percentage of water...so technically water is the solute here. Nevertheless, I realize that the 93% pertains to the concentration of nitric acid. Could someone review for me how to look at this, and how to change mass/mass % to molarity of the solution in general, but at least for this particular example? The molar mass/molecular weight of HNO3 is ~63.--...just making this as easy to answer as possible for that brave soul. Many thanks!
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Answer:
density ( g/L) x 93 / 100 = g/L of HNO3 in the solution g/L / Molar mass HNO3 => Molarity
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