How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2 ⋅ 0 M HNO 3 ? The concentrated acid is 70 % HNO 3.

Question

How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2 ⋅ 0 M HNO 3 ? The concentrated acid is 70 % HNO 3. (A) 90.0 g conc. HNO3 (B) 70.0 g conc. HNO3 (C) 54.0 g conc. HNO3 (D) 45.0 g conc. HNO3

Tardigrade Admin · Accepted Answer

The number of moles of nitric acid can be obtained by multiplying the molarity with volume

M \times V =

Moles of

H N O_{3} = \frac{250 \times 2}{1000} = 0.5

The mass of nitric acid can be obtained by multiplying the number of mols with molar mass and dividing with percentage concentration.

∴ H N O_{3}

required

= 0.5 \times 63 \times \frac{100}{70} = 45 g

Thus

45.0 g

conc.

H N O_{3}

of concentrated nitric acid solution should be used to prepare

250 m L

of

2.0 M H N O_{3}

.

Q. How many grams of concentrated nitric acid solution should be used to prepare $250 m L$ of $2 \cdot 0 M H N O_{3}$ ? The concentrated acid is $70% H N O_{3}$ .

$90.0 g$ conc. $H N O_{3}$

$70.0 g$ conc. $H N O_{3}$

$54.0 g$ conc. $H N O_{3}$

$45.0 g$ conc. $H N O_{3}$

Q. How many grams of concentrated nitric acid solution should be used to prepare 250mL of 2⋅0MHNO3​ ? The concentrated acid is 70%HNO3​.

90.0g conc. HNO3​

70.0g conc. HNO3​

54.0g conc. HNO3​

45.0g conc. HNO3​

Q. How many grams of concentrated nitric acid solution should be used to prepare $250 m L$ of $2 \cdot 0 M H N O_{3}$ ? The concentrated acid is $70% H N O_{3}$ .

$90.0 g$ conc. $H N O_{3}$

$70.0 g$ conc. $H N O_{3}$

$54.0 g$ conc. $H N O_{3}$

$45.0 g$ conc. $H N O_{3}$