How Do You Calculate Molality and Mole Fraction in Aqueous Nitric Acid?

AI Thread Summary
To calculate molality and mole fraction in aqueous nitric acid, first recognize that aqueous nitric acid consists of nitric acid (HNO3) as the solute and water (H2O) as the solvent. Given the density of 1.42 g/mL and a concentration of 16.0 mol/L, you can derive the mass of nitric acid and the mass of water needed for calculations. Molality is determined by the moles of solute per kilogram of solvent, while mole fraction is the ratio of moles of solute to the total moles of solute and solvent combined. Understanding the relationship between these values is crucial for solving the problem effectively. Clarifying these concepts will help in grasping the calculations involved.
n77ler
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Ok so I just started this course and we have to so review from first year stuff but I am completely lost and have no idea how to do the questions. There are a bunch so could someone just run through one with me please?

Commercial aqueous nitric acid has a density of 1.42g/mL and is 16.0mol/L HNO_3(aq). Calculate the molality, mass % and mole fraction of the HNO_3 present.

I don't understand because I thought there needed to be a solute and a solvent but here it seems like its asking about just one thing.
 
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Aqueous nitric acid means nitric acid (solute) dissolved in water (solvent). The term aqueous means that the solvent is water.
 
ok so HNO_3 + H_2O -----> NO_3- + H_3O+

Im sitll confused how the initial values are linked I'm getting extremely frustrated I'm falling behind because I cannot figure out the basics. PLease go through it with me!
 
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