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+.
If it is a solution its color is blue (but a bit green) . If it in solid state its color is greenish blue.
Red if you mean copper (I) oxide. Black if you mean copper (II) oxide
Copper Chloride is a light brown colour in its anhydrous (dry) state and if allowed to absorb moisture from the atmosphere turns to a bluey-green coloured dihydrate.
The oxide CuO is black.
CuO + 2 HCl -> CuCl2 + H2O Please see the link.
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
CuCl2 + H2S --> CuS + 2HCl Yes, this is the balanced equation here.
Copper dichloride
Under normal conditions CuCl2 can exist in either a solid state or in aqueous solution.
green
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.
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.
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.
CuO + 2 HCl -> CuCl2 + H2O Please see the link.
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)
Copper carbonate powder is a bluish green. When colorless sulphuric acid is added, the resulting solution has a slightly diluted color and a bunch of bubbles appear, making the color a lighter bluish green. However, when this solution is introduced to a flame (which would ordinarily be yellow), the flame burns green.
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.
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.