10 8. 7
presene
(a) T
(b)
(c)
collected in the U-tube.
(c) Name the colourless gas.
(d)
Write an equation for the reaction between ammonia and lead(II) oxide.
(e) State one industrial use of ammonia.
3. Explain the following:
(a) Nitric(V) acid is usually kept in dark brown bottles.
(b) Nitric(V) acid is often yellow in colour.
4. Aqueous ammonia was added to copper(II) sulphate solution dropwise until in
excess.
(a)
What observations were made?
(b) Write down the ionic equations representing the observations mentioned in
(a).
5. Calculate the volume of oxygen that would be obtained from the decomposition of
21.25 g of sodium nitrate at s. t.p. (1 mole of a gas occupies 22.4 dmº at s. t.p.)(N=14,
Na=23, 0 = 16).
6. What would be observed if the following tests were carried out on iron(II) sulphate
solution:
(a)
A little aqueous ammonia is added to iron(II) sulphate solution.
(b) A few drops of concentrated nitric(V) acid are added to iron(II) sulphate
solution and warmed gently.
(C) Excess aqueous ammonia is added dropwise to the mixture in (a) above.​