PART 1: Testing for the Presence of Sulphate Ions
REQUIREMENTS
Apparatus: 1 x comboplate ® ; 6 x thin stemmed propettes.
Chemicals: Sulphuric acid (H
2
SO
4
(aq)) [1.0 M]; Sodium hydrogencarbonate solution (NaHCO
Zinc nitrate solution (Zn(NO
3
)
2
Barium chloride solution (BaCl
(aq)) [0.5 M]; Hydrochloric acid (HCl(aq)) [11 M];
2
(aq)) [0.5 M]; Tap water.
If any acid is spilt on the skin thoroughly rinse the affected area with water.
PROCEDURE
3
(aq)) [0.5 M];
1.
2.
Use a clean propette to add 5 drops of tap water into well A1.
Add 5 drops of the following solutions: sulphuric acid (1.0 M) into well A2, sodium hydrogencarbonate (0.5
3.
M) into well A3 and zinc nitrate (0.5 M) into well A4. Use a clean propette for each solution.
Add 3 drops of barium chloride solution into each of wells A1 to A4. (See Question 1)
2.
3.
4. Use a clean propette to add 1 drop of 11 M hydrochloric acid into each of wells A1 to A4. (See Question 5)
Rinse the wells of the comboplate ® with tap water and shake them dry before proceeding with part 2.
PART 2: Testing for the Presence of Halide Ions
REQUIREMENTS
Apparatus:
Chemicals:
1 x comboplate ®
Nitric acid (HNO
3
; 5 x thin stemmed propettes.
Sodium chloride solution (NaCl(aq)) [0.1 M]; Sodium bromide solution (NaBr(aq)) [0.1 M];
Sodium iodide solution (NaI(aq)) [0.1 M]; Silver nitrate solution (AgNO
(aq)) [2.0 M].
3
(aq)) [0.1 M];
PROCEDURE
1. Add 5 drops of sodium chloride solution into well A1, 5 drops of sodium bromide solution into well A2 and 5 drops of sodium iodide solution into well A3.
Add 2 drops of nitric acid (2.0 M) and 3 drops of silver nitrate solution into each of wells A1 to A3.
Observe what happens. (See Questions 1, 2)
Wash the comboplate ® with tap water and shake dry.
Testing for Sulphate and Halide Ions Page 1 of 4

QUESTIONS – PART 1
Q1. What do you observe when a solution of barium chloride is added to wells A1 to A4?
Q2. In which well/s do you observe a precipitate?
Q3. Write the chemical formula to represent any precipitate/s observed in wells A1 to A4.
Sodium chloride and zinc chloride are both soluble in water.
Q 4. Can the addition of a solution of barium chloride (as in the above procedure) serve as a test for the presence of sulphates in aqueous solutions? Give a reason for your answer.
Q 5. What do you observe when 11 M hydrochloric acid is added to wells A1 to A4?
Q 6. In which well/s do you now observe a precipitate?
Q 7. Write a chemical formula to represent any precipitate/s observed in the above wells, after the addition of
HCl(aq).
Q 8. Explain any change observed in wells A1 to A4 on adding the HCl(aq).
Q 9. On the basis of your observations, state how you would test for sulphate ions in solution.
Q10. How would you show by experiment that a solution contained both carbonate and sulphate ?
QUESTIONS - PART 2
Q 1. Prepare a table like Table 1 below.
Table 1
Q 2. Record your observations in the table.
Q 3. Did a chemical reaction occur in any of wells A1 to A3? Explain your answer.
Q 4. Write a balanced chemical equation to represent any reaction which occurred in wells A1 to A3.
Q 5. From your observations is it possible to distinguish which halide is present in solution by adding silver nitrate? Explain your answer.
Testing for Sulphate and Halide Ions Page 2 of 4

1. Chemicals
All of the required chemicals are listed in the worksheet. Tap water is also needed in Part 1.
2. Equipment
Most of the apparatus required can be found in a Basic or Advanced Microchemistry Kit.
4. Cautions
Please remember the following cautions and inform your students of all safety hazards:
11 M hydrochloric acid is extremely corrosive. 1.0 M sulphuric acid and 2.0 M nitric acid are also dangerous if not handled safely. If any acid is spilt on the skin, the affected area must immediately be rinsed with copious amounts of water. Severe burns must receive medical attention.
Never point a propette or a syringe containing acid upwards. A momentary lapse of concentration can result in a nasty accident. If any acid is squirted into the eye, immediately rinse the eye out under running water.
Always have a dilute solution of sodium hydrogencarbonate (household baking soda), or milk close by to apply to the injury. These substances will help neutralise the acid in the eye. The patient should be referred to a doctor.
Silver is an expensive metal. Solutions of silver nitrate are also expensive and should not be wasted!
5. Model Answers to Questions in the Worksheet
It is recommended that learners write down all of the questions and answers in their workbooks. If this is done, then the answers to questions do not have to be in full sentences. If the learners do not copy the questions into their workbooks, then answers should be written in full sentences. Note that some of the questions can only be answered by learners in higher grades. Word equations can be written instead of chemical equations where required.
PART 1: Testing for the Presence of Sulphate Ions
Q1. What do you observe when a solution of barium chloride is added to wells A1 to A4 ?
A1. Well A1: The solution remains clear.
Well A2: The solution turns milky.
Well A3: The solution turns milky.
Well A4: The solution remains clear.
Q2. In which well/s do you observe a precipitate ?
A2. Wells A2 and A3.
Q3. Write the chemical formula to represent any precipitate/s observed in wells A1 to A4.
Sodium chloride and zinc chloride are both soluble in water.
A3. BaSO
4
(s) in well A2 and BaCO
3
(s) in well A3.
Q4. Can the addition of a solution of barium chloride (as in the above procedure) serve as a test for the presence of sulphates in aqueous solutions ? Give a reason for your answer.
A4. No. This is because the carbonate as well as the sulphate formed a white precipitate on addition of barium chloride solution.
Q5. What do you observe when 11 M hydrochloric acid is added to wells A1 to A4?
A5. Well A1: The solution remains clear.
Well A2: The solution remains milky.
Well A3: Bubbles can be seen. A clear solution forms.
Well A4: The solution remains clear.
Testing for Sulphate and Halide Ions Page 3 of 4

Q6. In which well/s do you now observe a precipitate ?
A6. Well A2.
Q7. Write a chemical formula to represent any precipitate/s observed in the above wells, after the addition of
HCl(aq).
A7. BaSO
4
(s).
Q8. Explain any change observed in wells A1 to A4 on adding HCl(aq).
A8. When hydrochloric acid is added to well A3 the barium carbonate precipitate reacts forming gaseous carbon dioxide (CO
2
(g)), water and barium chloride. The barium chloride is soluble in water and so the precipitate is observed to “disappear”.
Q9. On the basis of your observations, state how you would test for sulphate ions in solution.
A9. To test for sulphates in solution add hydrochloric acid followed by barium chloride. A white precipitate forms if sulphate is present.
Q10. How would you show by experiment that a solution contained both carbonate and sulphate ?
A10. Barium chloride solution could be added first. If a white precipitate forms it would indicate the presence of either carbonate or sulphate or both. Thereafter hydrochloric acid could be added. If the precipitate partly dissolves and bubbles of gas form, this indicates carbonate and sulphate.
PART 2: Testing for the Presence of Halide Ions
Q1. Prepare a table like Table 1 below.
A1. Table 1
Well
A1
Halide solution
NaCl(aq)
Initial appearance
colourless
Final appearance
white precipitate
A2 NaBr(aq) colourless light yellow
precipitate
A3 NaI(aq) colourless yellow precipitate
Q2. Record your observations in the table.
A2. See Table 1.
Q3. Did a chemical reaction occur in any of wells A1 to A3 ? Explain your answer.
A3. Yes. A precipitate was formed in each well. This is evidence that a chemical reaction occurred.
Q4. Write a balanced chemical equation to represent any reaction which occurred in wells A1 to A3.
A4. Well A1: NaCl(aq) + AgNO
Well A2: NaBr(aq) + AgNO
Well A3: NaI(aq) + AgNO
3
3
3
(aq)  AgCl(s) + NaNO
(aq)  AgBr(s) + NaNO
(aq)  AgI(s) + NaNO
3
3
(aq)
3
(aq)
(aq)
Q5. From your observations is it possible to distinguish which halide was present in solution by adding silver nitrate ? Explain your answer.
A5. Yes. The precipitate that formed in each well had a different colour. Silver chloride is white, silver bromide is light yellow and silver iodide is deeper yellow.
Testing for Sulphate and Halide Ions Page 4 of 4