Problem: Given the concentration of a weak base solution and a K b value for the weak base, what is the correct procedure to determine the pH of the solution? A.  Set concentration of weak base equal to [OH -], convert to [H3O+] and solve for pH B.  Convert Kb to Ka and use a table to find the equilibrium concentration of [H 3O+] and solve for pH C.  Convert Kb to Ka and use pH = pKa + log(base / acid) D.  Use a table to find the equilibrium concentration of the conjugate acid which is equal to [H  3O+] and solve for pH E.  Use a table to find the equilibrium concentration of [OH -], convert to [H3O+] and solve for pH

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Given the concentration of a weak base solution and a K b value for the weak base, what is the correct procedure to determine the pH of the solution?

A.  Set concentration of weak base equal to [OH -], convert to [H3O+] and solve for pH

B.  Convert Kb to Ka and use a table to find the equilibrium concentration of [H 3O+] and solve for pH

C.  Convert Kb to Ka and use pH = pKa + log(base / acid)

D.  Use a table to find the equilibrium concentration of the conjugate acid which is equal to [H  3O+] and solve for pH

E.  Use a table to find the equilibrium concentration of [OH -], convert to [H3O+] and solve for pH

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