# chemistry

posted by .

A commercial sample of concentrated aqueous nitric acid (HNO3) is 18.2% nitric acid base mass and has a density of 1.12 g/mL.

(a) What is the molarity (M) of the HNO3 solution?

(b) What is the molality (m) of the HNO3 solution?

--------

I know that....

(a) molarity = moles of solute/liters of solution

(b) molality = moles of solute/kg of solvent

But, I don't know how to find the moles of HNO3 (63 amu) with the information I have been given.

• chemistry -

assume some volume of the acid (it wont matter, it divides out).

Assume a volume of 2liters.

massnitric=.182*density*volume and you know density, and volume.
Now compute the moles of nitric given mass and its mole mass.

• chemistry -

So then the mass would equal .407 g?

And that would be .401/63 = .0065 mol?

Is that correct so far?
I don't really understand how I am able to just pic a random value for volume. The volume effects the mass, which effects the moles, right?

• chemistry -

You are not correct so far. I think you must have multiplied 2 L x 0.182 x 1.12. Note that the density is in g/mL so the units don't come out right.

## Similar Questions

1. ### Chemistry

A sample of conc. nitric acid has a density of 1.41g/ml and contains 70% HNO3 by mass. What mass of HNO3 is present per L of solution?
2. ### chemistry

A 116.9 g sample of nitric acid solution that is 70.0% HNO3 (by mass) contains how many moles of HNO3?
3. ### Chemistry

A solution is prepared by adding 50.3 mL of concentrated hydrochloric acid and 16.6 mL of concentrated nitric acid to 300 mL of water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH -], and the pH for this …
4. ### Chemistry

A solution is prepared by adding 47.3 mL of concentrated hydrochloric acid and 16.3 mL of concentrated nitric acid to 300 mL of water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH -], and the pH for this …
5. ### chemistry

Given 50 ml of concentrated nitric acid.The density of the concentrated acid is 1.42 g/ml and is 70% HNO3 by wt. Calc. the molality of the conc. acid.
6. ### chemistry

Given 50 ml of concentrated nitric acid.The density of the concentrated acid is 1.42 g/ml and is 70% HNO3 by wt. Calc. the molality of the conc. acid.
7. ### chemistry

The density of 19.0% by mass of nitric acid, HNO3 is 1.11 g cm-3. Calculate the volume (dm3) of acid needed to prepare 2.00 dm3 of 3.00 mol dm-3 HNO3 solution. (FW HNO3 = 63 g/mol)
8. ### chemistry

An aqueous solution of nitric acid is standardized by titration with a 0.121 M solution of calcium hydroxide. If 24.5 mL of base are required to neutralize 15.4 mL of the acid, what is the molarity of the nitric acid solution?
9. ### Chemistry

Concentrated nitric acid is 70% HNO3 and 14.7 M. What is the density of the solution?
10. ### chemistry

How many milliliters of concentrated nitric acid, HNO3, 70 % (wt/wt) are required to prepare 1 liter of 0.250 M solution?

More Similar Questions