26. Concentrated nitric acid used as a laboratory reagent is usually 69%by mass of nitric acid . Calculate the volume of the solution which contained 23 g of nitric acid . Density of conc. nitric acid is 1.41 g/cm3.

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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?

Q. Calculate the concentration of nitric acid in moles per litre in a sample which has a density.1.41 g/ml and the mass Y. of nitric acids is 69Y.

Q. Give reasons for the following:
(i) In laboratory preparation of nitric acid all the apparatus including cork should be made up of glass.
(ii) Commercial nitric acid is yellow in colour, but when it is diluted with water, it turns colourless.
(iii) Aluminium does not react with nitric acid of any concentration.
(iv) Conc. nitric acid renders iron passive.
(v) Nitric acid is used in purification of gold.
(vi) Aqua regia dissolves gold and platinum.
(vii) Nitric acid usually does not yield hydrogen from acids.
(viii) Lightning is a blessing in disguise.
(ix) Concentrated nitric acid is brown in colour.
(x) Concentrated nitric acid is a stronger oxidizing agent.

QUESTION 2.4

Concentrated nitric acid used in laboratory work is $68%68\%$ nitric acid by aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504 g $mL^{-1}$ ?

Q. (a) Write a balanced chemical equation for the laboratory preparation of nitric acid.
(b) In the preparation of nitric acid from

K N O_{3}

, concentrated hydrochloric acid is not used in place of concentrated sulphuric acid. Explain why.
(c) Conc. nitric acid prepared in laboratory is yellow in colour. Why? How is this colour removed? [4 MARKS]

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