What is the pH of 1M Cu(OH)Cl solution in water?

Lex thinks that you know the concentration of OH- ion, and that it is 1M. That simply is not the case. That would be assuming that Cu(OH)Cl completely ionizes. Instead, Cu(OH)Cl is INSOLUBLE in water. It is soluble in acids, to give Cu2+, Cl- and water.

The bottom line is that, along with Lex's answer, the entire question is bogus. It is impossible to have a solution of Cu(OH)Cl, let alone one with a concentration of 1M.

well you know the conc of OH- ...

and due to the kw of water being [H+] * [OH-] = kw = 1*10^-14

all you have to do is work out the conc of H+

so [H+] = (1*10^-14)/[OH-] = (1*10^-14)/1

and pH = -log( [H+] )

so pH = -log (1*10^-14)

=14

Depends on how much H2O you got