Common commercial acids and bases are aqueous solutions with the following properties.
Density (g/cm3) Mass Percent of Solute
Hydrochloric acid 1.19 38
Nitric acid 1.42 70
Sulfuric acid 1.84 95
Acetic acid 1.05 99
Ammonia 0.90 28
Calculate the molarity, molality, and mole fraction of each of the preceding reagents.
This is what I'm trying to do
I convert each density into (g/L). For the HCl Acid, that would be 1190 g/L... Since its mass percent is 38%, I multiply 1190g by .38, which equals 452.2g, which should be the mass HCl acid. I then convert that to moles, which becomes 12.40mol. 12.40mol/1L is 12.40M
Am I correct?