There is no simple answer. Cu+ and Cl- forms several complexes. The speciation depends on pH, ionic strength, concentrations. Cu+ is unstable in water , 2 Cu+ -> Cu2+  +   Cu(0) 

Copper does not exist as Cu+. It is presented as Cu2 ++ (cuprous) and Cu++ (cupric). Please be specific in your question which information you want to know.

Thank you Parashuram and Yurii

I know Copper canot be as single ion and there are lots of componds in water aqeuous, but for this reaction: [Cu++] + [2cl-] = [cucl2] for variety of temperatures, how can I find thermodynamic properties, i think there should be a way. In tables and books i have seen, there is only enthalpy of formation of each substance which doesnt work for me. So, I would appreciate if you let me know more about your viewpoints on this. 

Regards

Reza

I'm confused what are you asking for? Cu(I) or Cu(II) complexes?

I'm also confused by Parashuram's statement:"  It is presented as Cu2 ++ (cuprous) and Cu++ (cupric)." What is this "Cu++(cupric)?"

See for Cu(I)

Experimental study of copper(I) chloride complexing in hydrothermal solutions at 40 to 300 degrees C and saturated water vapor pressure

By:Xiao, ZF (Xiao, ZF); Gammons, CH (Gammons, CH); Williams-Jones, AE (Williams-Jones, AE)

GEOCHIMICA ET COSMOCHIMICA ACTA

Volume: 62

Issue: 17

Pages: 2949-2964

DOI: 10.1016/S0016-7037(98)00228-2

Published: SEP 1998

View Journal Information

Abstract

The solubility of Cu phases was measured in vapor-saturated aqueous HCl/NaCl solutions at temperatures ranging from 40 to 300 degrees C, total chlorideconcentration from 0.01 to 1 m, and pH from 0 to 3.5. For temperatures up to and including 150 degrees C, CuCl(S) was used as the solid reactant. At higher temperatures, foils of metallic Cu and Ag were used. Silver was added as a redox sensor, as the equilibrium constants describing dissolution of this metal aschloride complexes are already known to high precision. Copper was found to dissolve primarily as CuCl(aq), CuCl2-, and CuCl32-. Data collected from the experiments were regressed to determine the following equilibrium constants as functions of temperature (K):

Cu-(s) + 1/40(2(g)) + H+ + Cl- = CuCl(aq) + 1/2 H2O(1),

log K-1 = 0.1316*(1000/T)(2) + 2.865*(1000/T) + 4.4243, R-2 = 0.9958;

Cu-(s) +/- 1/40(2(g)) + H+ + 2Cl(-) = CuCl2- + 1/2 H2O(1),

log K-2 = 1.0981*(1000/T)(2) - 2.2961 *(1000/T) + 12.916, R-2 = 0.9896;

Cu-(s) + 1/40(2(g)) + H+ + 3Cl(-) = CuCl32- + 1/2H(2)O((1)),

log K-3 = 2.2704*(1000/T)(2) -8.7646*(1000/T) + 20.643, R-2 = 0.9941.

These equations can be used to calculate equilibrium constants at temperatures up to 350 degrees C and vapor saturated pressure.

Our results at T < 150 degrees C agree well with those published by other researchers, but the agreement is variable for results at T > 150 degrees C. At higher temperatures, our data for CuCl2- are in accord with those of Var'yash (1992), whereas our data for CuCl(aq) deviate significantly from the results of Crerar and Barnes (1976). The agreement with published theoretical estimates of the formation constants for Cu(I) chloride complexes (Helgeson, 1969; Ruaya, 1988; Sverjensky et al., 1997) is not good, especially at T > 200 degrees C.

The solubility of chalcopyrite was calculated for a variety of conditions. For unit activity of Cl-, pH between 3 and 5, and oxygen and sulfur fugacity buffered by the assemblage pyrite-pyrrhotite-magnetite, Cu is transported mainly as CuCl2-, and has a solubility of 212 moles/kg (13.5 ppm) at 350 degrees C and pH = 3. Chalcopyrite will deposit in response to an increase in pH, or decreases in a(Cl)-, temperature, and oxygen fugacity. Calculations of the solubility of chalcopyrite in seafloor hydrothermal systems show that the Cu-rich zones in volcanogenic massive sulfide deposits form at temperatures > 250 degrees C and that cooling and/or pH increase are the most Likely depositional controls. Below 250 degrees C, chloride brines are incapable of transporting significant quantities of Cu unless conditions are unusually oxidized. Copyright (C) 1998 Elsevier Science Ltd.

Additionally you can find the data on copper aqueous solutions in

Balashov V.N., Schatz R.S., Chalkova E., Akinfiev N.N., Fedkin M.V., and Lvov S.N., (2011) CuCl Electrolysis for Hydrogen Production in the Cu-Cl Thermochemical Cycle, J. Electrochem. Soc., 158(3), p. B266 – B275.

Weihua Liu, D.C. McPhail (2005) Thermodynamic properties of copper chloride complexes and copper transport in magmatic-hydrothermal solutions, Chemical Geology, 221, p. 21-39

The Helgeson thermodynamic package SUPCRT92 (Johnson, J.W., Oelkers, E.H. and Helgeson, H.C., 1992. SUPCRT92: A software package for calculating the standard molal thermodynamic properties of minerals, gases, aqueous species, and reactions from 1 to 5000 bar and 0 to 1000 °C. Comp. Geoscience, 18: 899-947.) has data on aqueous Cu+ (conventional ion form) and Cu++ .

Hall, Derek M.; Akinfiev, Nikolay N.; LaRow, Eric G.; et al. (2014)

Thermodynamics and Efficiency of a CuCl(aq)/HCl(aq) Electrolyzer,

ELECTROCHIMICA ACTA Volume: 143 Pages: 70-82

Akinfiev, N. N.; Zotov, A. V. (2010) Thermodynamic description of aqueous species in the system Cu-Ag-Au-S-O-H at temperatures of 0-600 degrees C and pressures of 1-3000 bar

GEOCHEMISTRY INTERNATIONAL Volume: 48 Issue: 7 Pages: 714-720

Thank you Dr. BValashov, I really appreciate what you shared with me. No doubt Pennsylvania univ is leader in CuCl electrolyzer, I will use lots of publications as reference.  

Wishes

Reza