11.3. Some reactions of the halide ions
A subsection of Chemistry, 9701, through 11. Group 17
Listing 10 of 171 questions
Concentrated sulfuric acid may be used in a school or college laboratory to produce hydrogen chloride by reaction with solid chlorides such as sodium chloride. What will be seen when concentrated sulfuric acid is carefully added to solid sodium chloride? Write a balanced equation for this reaction. Solutions of both H2SO4 and HCl are strong acids. What is meant by the term strong acid ? If the same reaction is carried out with solid sodium iodide and concentrated sulfuric acid, hydrogen iodide is not produced. State one observation you would make when carrying out this reaction with solid sodium iodide. Explain why hydrogen iodide is not a product of this reaction. Aqueous silver nitrate and aqueous ammonia are used to test for the presence of halide ions. Aqueous silver nitrate is slowly added to aqueous sodium chloride and the resulting mixture is then shaken with an excess of aqueous ammonia. Describe what you would observe at each stage of this process. Write balanced equations, with state symbols, for all reactions that occur in this process. The same process of adding aqueous silver nitrate followed by an excess of aqueous ammonia is repeated using aqueous sodium iodide instead of aqueous sodium chloride. State two differences that would be observed with aqueous sodium iodide.
9701_w12_qp_23
THEORY
2012
Paper 2, Variant 3
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The diagram below shows an incomplete experimental set-up needed to measure the Ecell of a cell composed of the standard Cu2+/Cu electrode and an Ag+/Ag electrode. copper electrode solution A electrode B saturated solution of AgCl solid AgCl State the chemical composition of solution A, electrode B. Complete the diagram to show the whole experimental set-up. The above cell is not under standard conditions, because the [Ag+] in a saturated solution of AgCl is much less than 1.0 mol dm–3. The Eelectrode is related to [Ag+] by the following equation. equation 1 Eelectrode = E electrode + 0.06 log[Ag+] Use the Data Booklet to calculate the E cell if the cell was operating under standard conditions. E cell = V In the above experiment, the Ecell was measured at +0.17V. Calculate the value of Eelectrode for the Ag+/Ag electrode in this experiment. Use equation 1 to calculate [Ag+] in the saturated solution. [Ag+] = mol dm–3 o o o Write an expression for Ksp of silver sulfate, Ag2SO4, including units. Ksp = units Using a similar experimental set-up to that illustrated opposite, it is found that [Ag+] in a saturated solution of Ag2SO4 is 1.6 × 10–2 mol dm–3. Calculate the value of Ksp of silver sulfate. Ksp = Describe how the colours of the silver halides, and their relative solubilities in NH3, can be used to distinguish between solutions of the halide ions Cl –, Br – and I –. Describe and explain the trend in the solubilities of the sulfates of the elements in Group II.
9701_w12_qp_41
THEORY
2012
Paper 4, Variant 1
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The diagram below shows an incomplete experimental set-up needed to measure the Ecell of a cell composed of the standard Cu2+/Cu electrode and an Ag+/Ag electrode. copper electrode solution A electrode B saturated solution of AgCl solid AgCl State the chemical composition of solution A, electrode B. Complete the diagram to show the whole experimental set-up. The above cell is not under standard conditions, because the [Ag+] in a saturated solution of AgCl is much less than 1.0 mol dm–3. The Eelectrode is related to [Ag+] by the following equation. equation 1 Eelectrode = E electrode + 0.06 log[Ag+] Use the Data Booklet to calculate the E cell if the cell was operating under standard conditions. E cell = V In the above experiment, the Ecell was measured at +0.17V. Calculate the value of Eelectrode for the Ag+/Ag electrode in this experiment. Use equation 1 to calculate [Ag+] in the saturated solution. [Ag+] = mol dm–3 o o o Write an expression for Ksp of silver sulfate, Ag2SO4, including units. Ksp = units Using a similar experimental set-up to that illustrated opposite, it is found that [Ag+] in a saturated solution of Ag2SO4 is 1.6 × 10–2 mol dm–3. Calculate the value of Ksp of silver sulfate. Ksp = Describe how the colours of the silver halides, and their relative solubilities in NH3, can be used to distinguish between solutions of the halide ions Cl –, Br – and I –. Describe and explain the trend in the solubilities of the sulfates of the elements in Group II.
9701_w12_qp_42
THEORY
2012
Paper 4, Variant 2
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