1. Acetic acid (CH3COOH) is a weak acid that reacts with water to form the acetate ion (CH COO). Write out the balanced reaction, and identify the acid, base, conjugate acid, and conjugate base. The equilibrium constant, K, for the above reaction is 1.8x10. If you add 1.31 g of acctice acid (FW-60.5 g/mol) to 24.2 mL of water, what are the equilibrium concentrations of acetic acid and acetate? What is the pH? 2. 3. The acetate ion is the conjugate base of acetic acid (CH,COOH), which is a weak acid with a pKa -4.74. Write out the balanced reaction when sodium acetate dissolves in water, and identify the acid,base, conjugate acid, ad conjugate base. What is the equilibrium constant for this reaction? 4. If you add 1.72 g of sodium acetate (FW-82.0 g/mol) to 28.7 mL of water, what are the equilibrium concentrations of acetic acid and acetate? What is the pH? 5. Hypoiodous acid (HOD is an extremely weak acid, with Ka-2x10Use an ICE table to find the pH of a 10 M solution of HO, ignoring any H,O' from the autoionization of water. Does this answer make sense? 6. Now, use an ICE table to find the pH of a 10 M solution of HOI, accounting for any H,O from the autoionization of water. Does this pH value make sense? 7. Use an ICE table to find the equilibrium [H,O'] and [OH] values from the autoprotolysis of water, using the [H,O] value you calculated above as the initial [H,O']. How does this affect pH?