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Bond [772]
2 years ago
7

The procedure calls for 2.0 ml of concentrated nitric acid. how many moles is this?

Chemistry
1 answer:
natka813 [3]2 years ago
8 0

Answer:

ρHNO₃= 1.51 g/cm3

ρ = m/V

m = ρ x V

m = (1.51 g/cm3)(2 cm3)= 3.02 g de HNO₃

n = m/PM = 3.02 g/63.01 g/mol = 0.0479 mol de HNO₃

Explanation:

2 mL of concentrated nitric acid equals 0.0479 mol

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The measurements below were made on four different balances:
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Explanation:

Hello!

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Question 27
3241004551 [841]

Answer:

24.9mL of the stock solution are required

Explanation:

To solve this question we have to find, as first, the moles of HCl that we need to prepare the desire solution. These moles are taken from the stock solution as follows:

<em>Moles diluted solution:</em>

500.0mL = 0.5000L * (0.613mol / L) = 0.3065 moles HCl

As these moles comes from the 12.3M HCl solution, the volume that we need of the stock solution is:

<em>Volume stock solution:</em>

0.3065 moles HCl * (1L / 12.3moles) = 0.0249L 12.3M HCl =

<h3>24.9mL of the stock solution are required</h3>
3 0
3 years ago
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