Basic Copper Chloride(WSDTY) compounds or ions at intermediate oxidation states can undergo disproportionation, a process in which a compound undergoes an autoredox reaction(where the same substance is simultaneously oxidized and reduced) to produce higher and lower oxidation states than the original. Combining equations 1.1and 1.2, copper disproportionates when in the state.
According to Malyszko and Kaczor, the equilibrium constant is determined by measuring the equilibr ium concentrations of Cu(I) and Cu(II). The equilibrium in equation 1.5(Kr= 106) favors the formation of Cu2+ under standard aqueous conditions. If the concentration of Cu+ is decreased, the equilibrium (Equation 1.5) is expected to shift to the right. If the concentration of Cu2+ is decreased, then the equilibrium is expected to shift to the left. Changing the ligands attached to copper changes the distribution of the equilibrium concentrations of Cu+and Cu2+.
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