CuCl2(s) = Cu^2_(aq) + + 2Cl^-(aq)
In solution the chloride anions )Cl^-) are colourless ; see also dissolved common salt (NaCl)
So it must be the copper cations (Cu^2+) that gives the colour blue.
When solid CuCl2 (copper(II) chloride) is mixed with water and dissolves to form a clear liquid, CuCl2 is referred to as a solute. In this solution, it dissociates into copper ions (Cu²⁺) and chloride ions (Cl⁻), resulting in an aqueous solution. The clear liquid formed is known as an aqueous solution of copper(II) chloride.
20.2 g of CuCl2 = .1502 mol CuCl2 M=mol/L M=.1502 mol/L
Copper is corroded in a sodium chloride solution; CuCl2 is formed.
Copper is dissolved:2 FeCl3 + Cu = 2 FeCl2 + CuCl2
The product of Cu + Cl2 reacting to form CuCl2 is copper(II) chloride. In this reaction, the copper (Cu) reacts with chlorine (Cl2) to form copper(II) chloride (CuCl2) as the product.
When NaSO3 is added to CuCl2 solution, a white precipitate of CuSO3 forms. Copper(II) sulfite is insoluble in water, causing it to precipitate out of the solution.
CuCl2 does NOT burn per se. However, when CuCl2 is dissovled in water in to Cu^2+ ions and Cl^- ions. Pass a ni-chrome or platinum wire through the solution, and then pass the wire through a Bunsen Burner flame. The flame colour will becomes a beautiful Blue/Green colour.
Under normal conditions CuCl2 can exist in either a solid state or in aqueous solution.
The flame color of CuCl2 is blue-green. This color is often observed when copper compounds are heated in a flame.
Cu(CO3) + 2HCl --> CuCl2 + H2O + CO2 CuCl2 product, when dry is a yellow/brown powder. However, when wet it forms a co-ordination complex with the water in the solution: CuCl2.2H2O --> Cu(Cl)2(H2O)2 The electronic structure of transition metals and ligands cause visible colours. In this case the solution is blue/green in colour. If you dry the solution down you will get a blue/green powder. Drying further in a dessicator will give the yellow/brown anhydrous CuCl2.
20.2 g of CuCl2 = .1502 mol CuCl2 M=mol/L M=.1502 mol/L
Copper(II) chloride (CuCl2) is not a base; it is a salt that is composed of copper(II) cations and chloride anions. It is an ionic compound that can dissociate in solution to form copper ions and chloride ions.
First multiply .131ml and 7.95M to get the moles of Cucl2. (You will need this later) Then find the moles per 49.5ml diluted solution. (6.1g divided my molar mass) Then set both equal to each other Original mol/X = Diluted mol/49.5ml and solve for X This should work
The chemical equation for the reaction that occurs when zinc metal is added to a solution of copper II chloride is: Zn + CuCl2 -> Cu + ZnCl2.
Copper is corroded in a sodium chloride solution; CuCl2 is formed.
The anion in CuCl2 is chloride (Cl-).
To determine the volume of the Na3PO4 solution needed for complete reaction, we would first write a balanced chemical equation for the reaction between Na3PO4 and CuCl2. Then, use the molarity of CuCl2 and the stoichiometry of the reaction to calculate the volume of Na3PO4 required.