Question

Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504 g mL–1? (2 Marks)
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Answer 1

Answer:

Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504 g mL–1? (2 Marks)

Write the formulas of. (i) Tetrahydroxozincate(II) (ii) Hexaamminecobalt(III) sulphate (iii) Potassium tetrachloridopalladate(II)Write the formulas of. (i) Tetrahydroxozincate(II) (ii) Hexaamminecobalt(III) sulphate (iii) Potassium tetrachloridopalladate(II

Answer 2

Answer:

The molar mass of nitric acid is 63 g/mol.

It is given that the nitric acid used in the laboratory is 68% by mass in aqueous solution.

100 g of solution contains 68 g of nitric acid or

68/63 =1.079 moles of nitric acid.

Density of solution is 1.504 g/mL.

100 g of solution corresponds to 100/1.504 =66.5 mL or 0.0665 L

Molarity of the solution is the number of moles of nitric acid present in 1 L of solution.

It is 1.079/0.0665 =16.22 M

Hence, the molarity should be 16.22 g/mL.

Explanation:

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