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Molarity

Find the volu...

Question

Find the volume of water (in mL) added to 50 mL concentrated nitric acid $H N O_{3}$
$(d = 1.52 g m l^{- 1}$ , 69% by mass) that forms diluted nitric acid ( $d = 1.15 g m L^{- 1}$ , 19% by mass $H N O_{3}$ ).

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Solution

Let volume of dilute solution that can be formed is V.
Mass of $H N O_{3}$ will be same before and after dilution
So, $V \times 1.15 \times 0.19 = 50 \times 1.52 \times 0.69$
$⟹ V = 240$ mL
Volume of water added = 240 - 50 = 190 mL.

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Similar questions

Q. Find the volume of water (in mL) added to 50 mL concentrated nitric acid

H N O_{3}

(d = 1.52 g m l^{- 1}

, 69% by mass) that forms diluted nitric acid (

d = 1.15 g m L^{- 1}

H N O_{3}

Q. 240 ml of diluted nitric acid (d = 1.15 g/ml, 19% by mass)

H N O_{3}

is to be prepared from conc.

H N O_{3}

(d =1.52 g/ml, 69% by mass). How much water has to be added (in mL) to the concentrated solution to achieve this?

Q. Determine the volume of dilute nitric acid (

d = 1.11

m L^{- 1}

19 %

H N O_{3}

) that can be prepared by diluting with water

50

H N O_{3}

d = 1.42

m L^{- 1}

69.8 %

Q. (a) Nitric acid cannot be concentrated beyond 68% by the distillation of a dilute solution of HNO₃. State the reason.
(b) How can 68% nitric acid be concentrated to 98% nitric acid?

Q. How many grams of concentrated nitric acid solution should be used to prepare

250 mL

2.0 M H N O_{3}

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70 % H N O_{3}

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