2(i)
The figure given below illustrates the apparatus used in the laboratory preparation of nitric acid.
(a) Name:
(b) Why should we use only glass apparatus in the laboratory preparation of nitric acid?
(c) Write an equation to show how nitric acid undergoes decomposition.
(d) What do you observe when copper is oxidized by concentrated nitric acid?
- (a)R (a liquid) and
- (b)S (a solid)
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(a)
- R — Concentrated sulphuric acid (H2SO4)
- S — Sodium nitrate (NaNO3) [potassium nitrate, KNO3, is also acceptable]
(b) Only glass apparatus is used because nitric acid vapours attack rubber and cork.
(c) 4HNO3 $\xrightarrow{\text{heat / light}}$ 4NO2 + 2H2O + O2
(d) Dense reddish-brown fumes of nitrogen dioxide are evolved and a blue solution of copper(II) nitrate is formed.
Cu + 4HNO3 [conc.] ⟶ Cu(NO3)2 + 2H2O + 2NO2