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mr Goodwill [35]
2 years ago
15

Calculate the mass of nitric acid required to make a 250mL solution with 2.40 ph

Chemistry
1 answer:
meriva2 years ago
3 0

The mass of nitric acid required to make the given solution is 0.0627 g.

The given parameters:

  • <em>Volume of the acid, V = 250 mL</em>
  • <em>pH of the acid, = 2.4</em>

The hydrogen ion (H⁺) concentration of the nitric acid is calculated as follows;

H^+ = 10^{-pH}\\\\H^+ = 10^{-2.4}\\\\H^+ = 0.00398

The molarity of the nitric acid is calculated as follows;

=  0.00398 \ H^+ \times \frac{1 \ M \ HNO_3}{1 \ H^+} \\\\= 0.00398 \ M

The number of moles of the nitric acid is calculated as follows;

moles = M\times L\\\\moles = 0.00398\ M \ \times \ \frac{250 \ mL}{1000} \\\\moles = 9.95 \times 10^{-4} \ mol.

The molar mass of nitric acid is calculated as;

HNO_3 = (1) \ + (14) \ + (16 \times 3) = 63 \ g/mol

The mass of the nitric acid contained in the calculated number of moles is calculated as;

mass = moles\  \times \ molar \ mass\\\\mass = 9.95\times 10^{-4} \ mol. \ \times \ 63 \ g/mol\\\\mass = 0.0627 \ g

Thus, the mass of nitric acid required to make the given solution is 0.0627 g.

Learn more about molarity of acids here: brainly.com/question/13864682

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