Use equilibrium equations to explain why Cu(Cl)2 is more soluble in a solution of sodium cyanide than in pure water, given that it forms the complex ion Cu(CN)42-.
CuCl2 is sparingly soluble in water give the solubility equilibrium,
CuCl2 <=> Cu2+ + 2Cl- --------------------(1)
In cyanide solution, Cu complexes with the cyanide ion and forms Cu(CN)42-
Cu2+ + 4CN- -> Cu(CN)42-
The dissolved CuCl2 forms Cu2+ which forms Cu(CN)42-, which affects the equilibrium shown in equation (1)
According to Le Chatelier's principle, if concentration of product in an equilibrium is reduced, then the forward reaction speeds up.
Here The forward reaction is the dissolution process. So as Cu2+ gets taken to form the complex, the equilibrium makes the forward reaction more fast, hence dissolution of Cu2+ happens and CuCl2 gets more dissolved in NaCN solution.
Use equilibrium equations to explain why Cu(Cl)2 is more soluble in a solution of sodium cyanide...
a) What molarity of NaOH can be added to a solution of 1.5 x 10-4M Mn(NO3)2, given the Ksp of Mn(OH)2 = 1.6 x 10-13 b) Use equilibrium equations to explain why Cu(Cl)2 is more soluble in a solution of sodium cyanide than in pure water, given that it forms the complex ion Cu(CN)42-.
Which salts will be more soluble in an acidic solution than in pure water? Explain why each salt is or is not more soluble in an acidic solution than in pure water. CuCl CsClO4 CaSO4 Be(OH)2 AlPO4
Could you explain why too? Thank you.
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