(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

Nitric acid is commercially available as a 72% ( w/ w) solution ( density, 1.42 g/cm3). How many milliliters of this reagent are needed to prepare 2.00 L of a 1.00M HNO3 solution?

2. Relevant equations

C%= (g HNO3/ g Solution) * 100

3. The attempt at a solution

So basically, I started with converting a mole of the solution to mL.

1 mol HNO3=44.37ml

But I feel like I need to first use the concentration to find how much reagent is in that 72%. so its .72g I assume that the reagent is contained in that solution.

so .72g of HNO3 in the solution is .507mL

but now I am stuck. How do I use that information to figure out what the mL of the reagent is needed to get 2L of 1 mol of HNO3

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