Co(H2O)6^2 + 4 Cl^‐1 (aq) ⇄ CoCl4^‐2 (aq) + 6 H2O (l) + 50 kJ
AgCl(s) = Ag+(aq) + Cl‐(aq)
1.6E-10 = (Ag^+)(Cl^-)
If the right side is only 1.6E-10, doesn't that mean there is much more solid than ions?
a)
Co(H2O)6^2 + 4 Cl^‐1 (aq) ⇄ CoCl4^‐2 (aq) + 6 H2O (l)
Rewrite the net ionic equation above including the energy term where appropriate. The Delta H for this reaction is +50 kJ/mol.
b)
Silver chloride (AgCl) is a white solid. For the equilibrium reaction AgCl(s) = Ag+(aq) + Cl‐(aq) The Ksp for AgCl = 1.6 * 10‐10. At equilibrium, would you expect to have more silver and chloride ions or more solid silver chloride?
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