Solution A contains the compound [Cu(H2O)6]Cl2 - AQA - A-Level Chemistry - Question 7 - 2017 - Paper 1
Question 7
Solution A contains the compound [Cu(H2O)6]Cl2.
1. State the type of bonding between the oxygen and hydrogen in this compound.
2. State why the chloride ions in th... show full transcript
Worked Solution & Example Answer:Solution A contains the compound [Cu(H2O)6]Cl2 - AQA - A-Level Chemistry - Question 7 - 2017 - Paper 1
Step 1
State the type of bonding between the oxygen and hydrogen in this compound.
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Answer
The type of bonding between the oxygen and hydrogen in the compound [Cu(H2O)6]Cl2 is covalent. This is because the bond is formed by the sharing of electrons between the oxygen and hydrogen atoms.
Step 2
State why the chloride ions in this compound are not considered to be ligands.
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Answer
The chloride ions are not considered to be ligands because they do not donate a lone pair of electrons to the central copper ion; instead, they form an ionic bond.
Step 3
Write an ionic equation for the reaction that occurs when solution A is converted into solution B and state the colour of solution B.
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Answer
The ionic equation for the reaction is:
[Cu(H2O)6]2++4NH3→[Cu(NH3)4]2++6H2O
The colour of solution B is deep blue or royal blue.
Step 4
Identify the blue-green solid C.
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Answer
The blue-green solid C is CuCO3, or copper carbonate.
Step 5
Identify reagent D and write an ionic equation for the reaction that occurs when the yellow-green solution is formed from solution A.
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Answer
Reagent D is HCl (hydrochloric acid). The ionic equation for the reaction is:
[Cu(H2O)6]2++4Cl−→[CuCl4]2−+6H2O
Step 6
Explain why colorimetry cannot be used to determine the concentration of solutions containing [CuCl2].
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Answer
Colorimetry cannot be used for solutions containing [CuCl2] because the solution is colorless. Colorimetry relies on the absorption of visible light, and since [CuCl2] does not absorb light in the visible region, this method cannot provide accurate concentration measurements.
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