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ad-work [718]
4 years ago
9

Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and has a density of 1.41 g/mL. How much conc

entrated solution would you take to prepare 1.00 L of 0.120 M HNO3 by mixing with water?
Chemistry
1 answer:
Marina CMI [18]4 years ago
8 0

Answer:

The answer to your question is: 9 .43 ml of HNO3 70.3%

Explanation:

Data

Purity: 70.3%

density = 1.41g/ml

Volume = 1 l

Concentration = 0.12 M

Molecular weight = 1 + 14 + (16 x 3) = 63 gr

               63 gr of HNO3 ------------------1 mol of HNO3  or IM

                           x           -------------------              0.12 M

x = 0.12M x 63 /1 = 7.65 g of HNO3

Now, calculate volume

        density = mass / volume    and volume = mass/density

                               volume = 7.65 / 1.41 = 6.63 ml of HNO3

Now, consider purity  (it's and inver rule of three)

                          6.63 ml -----------------  100%

                              x       -----------------  70.3 %

           x =  (6,63 x 100)/70.3 = 9.43 ml of HNO3

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