Test for Anions
Colours of some metal hydroxides
Testing for cations
Cations can be identified by their reactions with aqueous sodium hydroxide and aqueous ammonia
A precipitate is an insoluble solid.
When testing for cations, these precipitates only form when a metal ion in solution joins with hydroxide ions in solution to form an insoluble metal hydroxide
eg Cu2+ + 2OH- --> Cu(OH)2 (blue copper(II) hydroxide precipitate)
[Lead(II) ions can be distinguished from aluminium ions by the insolubility of lead(II) chloride.]
1. Which statement about salts is not correct?
a, salts are made by neutralising alkalis with acids
b. salts contain anions and cations
c. salts are made by dissolving metal oxides in acids
d. salts always contain water of crystallisation
2. An example of a salt which can be prepared by precipitation is
a. lead(II) nitrate
b. sodium carbonate
c. silver chloride
d. magnesium sulphate
3. A way of distinguishing dilute hydrochloric acid from dilute sulphuric acid is to
a. add universal indicator
b. add aqueous barium nitrate
c. add a metal carbonate
d. add magnesium ribbon
4. Which of these statements about solubility is true?
a. all sulphates are soluble in water except calcium and lead sulphate
b. all nitrates are insoluble in water except sodium and potassium nitrate
c. most metal oxides are soluble in water except those of Group I and II
d. most metal carbonates are soluble in water
5. Barium sulphate is insoluble in water. It is used in a 'barium meal' to allow X-ray studies of the intestines. It can be prepared by a precipitation reaction between two aqueous solutions. Which two substances would be suitable for preparing barium sulphate for use in X-ray radiography?
a. barium carbonate and sulphuric acid
b. barium chloride and sodium sulphate
c. barium oxide and potassium sulphate
d. barium nitrate and calcium sulphate
6. Which of these salts is best prepared by reaction with an acid and a base?
a. barium sulphate
b. copper(II) carbonate
c. magnesium sulphate
d. silver chloride
7. A solution of substance X gave a white precipitate when aqueous NaOH was added. However, when lead(II) nitrate solution was added to an acidified solution of X, a yellow precipitate formed. What is the correct identity of X?
a. calcium chloride
b. magnesium sulphate
c. sodium bromide
d. zinc iodide
8. Iron(III) hydroxide is precipitated out of solution when aqueous sodium hydroxide solution is added to iron(II) chloride solution.
Fe3+ (aq) + 3OH- (aq) --> Fe(OH)3 (s)
What is the minimum volume of 2 mol/dm3 aqueous NaOH required to precipitate the maximum amount of iron(III) hydroxide from 20cm3 of 1 mol/dm3 iron(III) chloride solution?
a. 10 cm3
b. 20 cm3
c. 30 cm3
d. 60 cm3
9. After acidification with dilute nitric acid, a colourless solution X reacts with aqueous silver nitrate to give a yellow precipitate. What could X be?
a. calcium iodide
b. copper(II) chloride
c. iron(II) iodide
d. sodium chloride
10. An element reacts with steam but not with cold water. Its oxide can be reduced by heating it with carbon. When it is placed in a solution containing iron(II) ions, a grey deposit is formed. The element is most likely to be
Structured Questions Worked Solutions
1. A student was given an aqueous solution analyse. It contains copper(II) chloride and aluminium nitrate.
a. Describe how he could detect the presence of chloride ions in the aove solution.
b. Name the precipitate(s) formed when excess aqueous ammonia is added to the above solution.
Add dilute nitric acid followed by aqueous silver nitrate.
A white precipitate will be seen in the presence of chloride ions
Add dilute nitric acid followed by aqueous lead(II) nitrate.
A yellow precipitate will be seen in the presence of chloride ions
2. W is an alkali and X is a salt. When the two solutions were mixed together, a reddish-brown precipitate Y was obtained. When a salt Z was added to solution W and heated, a pungent gas which turned moist red litmus blue was evolved. Suggest what could W, X, Y, and Z be.
W: Sodium hydroxide
X: Iron(III) chloride/sulphate/etc
Y: Iron(III) hydroxide
Z: Ammonium chloride/nitrate/etc
3. Give the name and formula of the ions present in each of the solutions X, Y and Z below -
a. Solution X gives a white precipitate when dilute hydrochloric acid and aqueous barium chloride are added to it.
b. An alkaline gas is given off when sodium hydroxide solution is added to the colourless solution Z and the mixture heated.
3a. sulphate ion (SO42-)
3b. Ammonium ion (NH4+)
4. A similar reagent is added to zinc carbonate and sample S to initiate both reactions A and B.
a. Identify A to F.
b. Write an ionic equation (with state symbols) for the formation of the yellow precipitate.
c. Describe a test for the pungent gas R.
d. Pungent gas R dissolves in water to form a solution. Describe the observations when a few drops of copper(II) sulphate solution is added to the solution.
A: lead(II) carbonate
B: dilute nitric acid
C: ammonia gas
D: carbon dioxide
E: lead(II) nitrate
F: lead(II) hydroxide
b. Pb2+ (aq) + 2I- (aq) ---> PbI2 (s)
c. Place two pieces of damp red and blue litmus papers at the mouth of the test tube. If the gas is ammonia, the damp red litmus paper will turn blue. A pungent gas will also be detected.
d. Blue precipitate is formed which dissolves in excess aqueous ammonia to form a dark blue solution.
6. In the experiment shown below, the gas X produced by the action of dilute sulphuric acid on the zinc granules was passed over two heated metallic oxides. A colourless liquid W was collected and the excess gas X was burnt off at Y.
ai. Name the reagent(s) required for Reaction A.
aii. Write down the chemical equation (with state symbols) for Reaction A.
bi. Give a possible identity of Sample S.
bii. Based on your answer in bi, write a chemical equation with state symbols for Reaction B.
ai. Hydrochloric acid
aii. ZnCO3 (s) + 2HCl (aq) ---> ZnCl2 (aq) + CO2 (g) + H2O (l)
bii. Zn (s) + 2HCl (aq) ---> ZnCl2 (aq) + H2 (g)
a. What is gas X? Write the ionic equation for the formation of the gas.
b. State what is observed of:
i. zinc oxide
ii. copper(II) oxide
Write equation(s) for any change observed.
c. Explain your observation made in bi and bii.
d. Give a chemical test to identify liquid W.
e. Suggest a suitable drying agent to be placed inside the drying bulb.
f. Why was the excess gas X burnt off at Y?
g. What precautions should be taken before the excess gas was lit?
Zn + 2H+ ---> Zn2+ + H2
bi. Zinc oxide turns from white to yellow.
bii. Copper(II) oxide turns from black to pink
CuO + H2 ---> Cu + H2O
c. Zinc is above hydrogen in the reactivity series so zinc oxide will not be reduced by hydrogen to zinc. Upon being heated, zinc oxide will change its colour from white to yellow.
Copper is below hydrogen in the reactivity series so copper(II) oxide will be reduced to form pink copper.
d. W is tested with anhydrous cobalt(II) chloride paper. If W is water, the cobalt(II) chloride paper will turn from blue to pink.
e. fused calcium chloride
f. Because hydrogen gas is flammable and a mixture of hydrogen and air is very explosive.
g. Ensure that there is no leakage in the apparatus.