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.
96%
114 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
The type of bonding between the oxygen and hydrogen in this compound is covalent.
Step 2
State why the chloride ions in this compound are not considered to be ligands.
99%
104 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
The chloride ions are not considered to be ligands because they do not donate a lone pair to the copper atom; instead, they are coordinated ionically.
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.
96%
101 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
The ionic equation for the reaction is:
[Cu(H2​O)6​]2++4NH3​→[Cu(NH3​)4​]2++6H2​O
The colour of solution B is deep blue or royal blue.
Step 4
Identify the blue-green solid C.
98%
120 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
The blue-green solid C is copper carbonate (CuCO3) or basic 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.
97%
117 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
Reagent D is hydrochloric acid (HCl). The ionic equation for the reaction is:
Cu2++4Cl−→[CuCl4​]2−
Step 6
Explain why colorimetry cannot be used to determine the concentration of solutions containing [CuCl2].
97%
121 rated
Only available for registered users.
Sign up now to view full answer, or log in if you already have an account!
Answer
Colorimetry cannot be used to determine the concentration of solutions containing [CuCl2] because the solution is colorless, which means it cannot absorb the visible light necessary for colorimetric analysis. Additionally, the electron configuration of the metal ion does not allow for any optical activity in this context.
![Solution-A-contains-the-compound-[Cu(H2O)6]Cl2-AQA-A-Level Chemistry-Question 7-2017-Paper 1.png](https://cdn.simplestudy.io/assets/backend/uploads/question/Question_7_2017_Chemistry_P1.jpg)
