A LevelChemistryAQAExam QuestionsAdvanced Inorganic ChemistryReactions of Ions in Aqueous Solution

Reactions of Ions in Aqueous Solution (AQA A Level Chemistry): Exam Questions

Exam code: 7405

4 hours31 questions

Select a download format for Reactions of Ions in Aqueous Solution

Scroll for more

Select an answer set to view for
Reactions of Ions in Aqueous Solution

Easy
Medium
Hard
1
1 mark

Which of the following is true about the bonding in metal-aqua ions?

  • Water molecules act as Brønsted-Lowry acids

  • Metal ions act as Brønsted-Lowry bases

  • Water molecules act as Lewis bases

  • Metal ions act as proton acceptors

Choose your answer

2
1 mark

Which of the following is true about metal-aqua ions?

  • All aqueous transition metal ions are neutral 

  • Transition metal ions with a +2 charge are acidic

  • Deprotonation occurs in all transition metal ions

  • Transition metal ions with a +3 charge are acidic

Choose your answer

3
1 mark

A white precipitate with some bubbles could be the observations in which of the following reactions?

  • CuCl2 + NH3

  • Al2(SO4)3 + Na2CO3

  • H2SO4 + Na2CO3

  • BaCl2 + Na2SO4

Choose your answer

4
1 mark

Aqueous iron(II) ions react with ammonia according to the following equation:

[Fe(H2O)6] 3+ (aq)  + 3NH3 (aq) →    Fe(H2O)3(OH)3 (s)  + 3NH4+ (aq)

In this reaction, what is the role of the ammonia?

 

Base

Nucleophile

Ligand

A

✓

✓

✓

B

✓

✓

⨯

C

⨯

✓

✓

D

✓

⨯

⨯

 

    Choose your answer

    5
    1 mark

    Copper(II) nitrate can undergo the following sequence of reactions:

     Cu left parenthesis NO subscript 3 right parenthesis subscript 2 space rightwards arrow with Step space 1 on top space space blue space solution space straight A space rightwards arrow with Step space 2 on top space space blue space precipitate space straight B space rightwards arrow with Step space 3 on top space dark space blue space solution space straight C

    The reagents needed to carry out steps 1, 2 and 3 could be

     

    Step 1

    Step 2

    Step 3

    A

    Excess H2O

    Drops of NaOH (aq)

    Drops of conc. HCl (aq)

    B

    Excess H2O

    Excess NH3 (aq)

    Drops of conc. HCl (aq)

    C

    Excess H2O

    Drops of NH3 (aq)

    Excess NH3 (aq)

    D

    Excess H2O

    Drops of NH3 (aq)

    Excess H2O

      Choose your answer

      1
      1 mark

      Iron(III) forms a complex ion [Fe(H2O)6]3+.

      What is the role of the water molecule in this species?

      • Brønsted-Lowry acid and Lewis base

      • Brønsted-Lowry base and Lewis base

      • Brønsted-Lowry base only

      • Lewis base only

      Choose your answer

      2
      1 mark

      Transition metal ions with the general formula, M3+, will often undergo hydrolysis reactions in water. One such ion is Fe(III) and the reactant side of the hydrolysis equation is:

       [Fe(H2O)6]3+    +   H2O      ⇌      -------------------      +     -------------------

      Which of the following correctly completes the equation?

      • [Fe(H2O)5(OH)]2+    +   H+

      • [Fe(H2O)5(OH)]3+    +   H3O+

      • [Fe(H2O)5(OH)]2+    +   H3O+

      • Fe(H2O)3(OH)3          +  3H+

      Choose your answer

      3
      1 mark

      Which of the following ions produces identical observations when sodium hydroxide or ammonia solutions are added until in excess?

      • [Fe(H2O)6]2+

      • [Al(H2O)6]3+

      • [Cu(H2O)6]2+   

      • [Co(H2O)6]2+

      Choose your answer

      4
      1 mark

      Chelation is the formation of complexes with multidentate ligands.

      Which of the following is true about chelation?

      • Stronger bonds are formed between the multidentate ligands and the central metal ions

      • The chelated complexes are more stable due to positive entropy changes

      • The number of entities decreases in chelation which favours the reaction

      • Negative enthalpy changes during chelation favour the reactions

      Choose your answer

      5
      1 mark

      Aqueous iron(III) ions react with sodium carbonate solution.

      What happens in the reaction?

       

      Observations

      Products

      A

      Brown precipitate

      Bubbles of gas

      Fe(H2O)3(OH)3

      CO2

      B

      Brown precipitate

      -

      Fe2(CO3)3

      -

      C

      Orange solution

      -

      [Fe(H2O)5(OH)]2+

      -

      D

      Brown precipitate

      Bubbles of gas

      Fe2(CO3)3

      CO2

       

        Choose your answer

        1
        1 mark

        Two possible reactions of hydrated chromium(III) hydroxide are shown below.

        6-3-aqa-a-level-chemistry-mcq-q1-hard

        Which statement about these reactions is correct?

        • Reaction 1 shows the hydrated chromium(III) hydroxide acting as a Brønsted–Lowry acid

        • Reactions 1 and 2 are examples of ligand substitution reactions

        • Reactions 1 and 2 display the amphoteric nature of hydrated chromium(III) hydroxide

        • Reaction 2 shows the hydrated chromium(III) hydroxide behaving as a Brønsted–Lowry base

        Choose your answer

        2
        1 mark

        Hexa-aqua solutions of transition metals in the +2 oxidation state, [M(H2O)6]2+ (aq), can react with excess aqueous ammonia to form various complexes.

        Which of the following statements about these reactions with excess aqueous ammonia is correct?

        • [M(H2O)6]2+ (aq) can form products that exist as stereoisomers

        • [M(H2O)6]2+ (aq) undergo full ligand substitution to form [M(NH3)6]2+ (aq)

        • [M(H2O)6]2+ (aq) forms products with the transition metal in the +3 oxidation state

        • [M(H2O)6]2+ (aq) can form precipitates of [M(H2O)4(NH3)2] (s)

        Choose your answer

        3
        1 mark

        The reactions of three different metal complexes with aqueous sodium hydroxide are shown in the table.

        Formula of complex ion

        Addition of small amount of NaOH (aq)

        Addition of excess NaOH (aq)

        [M(H2O)6]2+

        Coloured precipitate forms

        No further change

        [X(H2O)6]3+

        Coloured precipitate forms

        Precipitate dissolves

        [Q(H2O)6]3+

        White precipitate forms

        Precipitate dissolves

         

        Which statement about the metals is most likely to be true?

        • Q is not a transition metal

        • The [M(H2O)6]2+ complex will react with carbonate ions to produce carbon dioxide 

        • [X(H2O)6]3+ forms a precipitate with carbonate ions with the formula XCO3

        • [Q(H2O)6]3+ forms a coloured solution when excess aqueous ammonia is added

        Choose your answer

        4
        1 mark

        The pH of a 1.0 mol dm-3 solution of aluminium chloride is approximately 3, whereas the pH of a 1.0 mol dm-3 solution of iron(II) chloride is approximately 5.

        What is the best explanation for this?

        • The Al3+ has a greater charge density than the Fe2+ ion

        • The aluminium chloride solution contains more ions

        • The Al3+ ion has a greater nuclear charge than the Fe2+ ion

        • The aqueous Al3+ ion has a greater coordination number than the Fe2+ ion

        Choose your answer

        5
        1 mark

        Which of the options below shows the correct observation and chemical explanation for the reactions of a solution of iron(II) chloride?

         

         

        Substance added (in excess)

        Observation

        Explanation

        A

        Na2CO3 (aq)

        Green precipitate which redissolves to form a green solution

        Carbonate ions act as a base, removing H+ from the water molecules in the complex

        B

        NH3 (aq)

        Green precipitate which redissolves to form a green solution

        A ligand exchange reaction occurs  - ammonia displaces

        C

        Na2CO3 (aq)

        Green precipitate which does not redissolve; fizzing

        Carbonate ions act as a base, removing H+ from the water molecules in the complex. CO2 gas is also formed.

        D

        NH3 (aq)

        Green precipitate which does not redissolve

        Ammonia acts as a base, removing H+ from the water molecules in the complex

         

          Choose your answer