Hydrated copper sulphate is blue in color while anhydrous copper sulphate is white in color.
CuSO4 is white, the pentahydrate crystal (CuSO4.5H2O) and the aquous solution (Cu2+(aq) ions) are royal blue. So the color comes from the hydration of Cu2+.
Since copper (I) chloride has only limited solubility in water I will assume you mean copper (II) chloride, CuCl2. Then the ions will be Cu2+ and Cl-.
CuCl2(aq) + K2S(aq) --> CuS(s) + 2KCl(aq) K and Cl are spectators so the net ionic would be: Cu2+(aq) + S2-(aq) --> CuS(s)
In the reaction Zn + CuCl2 → ZnCl2 + Cu, CuCl2 is the oxidizing agent because it accepts electrons from Zn, causing zinc to be oxidized and copper to be reduced.CuCl2 itself gets reduced to Cu.
It is Copper chloride.It is written as Copper(ii) chloride.
When copper nitrate reacts with barium chloride, a white precipitate of barium nitrate is formed. Copper chloride remains in solution as ions. This reaction can be represented by the equation: Cu(NO3)2 + BaCl2 -> Ba(NO3)2 + CuCl2.
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.
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.
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
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.
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
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.
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.
As gaseous ammonia with solid coppersulfate: 2NH3(g) + CuSO4(s) --> Cu(NH3)2SO4(s) With water: [Cu(NH3)2]2+ complex-ions with SO42- ions in aquous solution (deep blue color)