1)

A buffer can be prepared by mixing two solutions. Determine if each of the following mixtures will result in a buffer solution or not.  

1) Mixing 100.0 mL of 0.1 M HCl with 100.0 mL of 0.1 M NaOH                              [ Select ]                       [“No, it will not result in a buffer solution.”, “Yes, it will result in a buffer solution.”]      

2) Mixing 100.0 mL of 0.1 M CH₃COOH with 100.0 mL of 0.05 M mol CH₃COONa                              [ Select ]                       [“Yes, it will result in a buffer solution.”, “No, it will not result in a buffer solution.”]      

3) Mixing 100.0 mL of 0.1 M NH₃ with 100.0 mL of 0.1 M NH₄Cl                              [ Select ]                       [“No, it will not result in a buffer solution.”, “Yes, it will result in a buffer solution.”]      

4) Mixing 100.0 mL of 0.1 M NH₃ with 100.0 mL of 0.05 M HNO₃                              [ Select ]                       [“No, it will not result in a buffer solution.”, “Yes, it will result in a buffer solution.”]      

5) Mixing 100.0 mL of 0.1 M NH₃ with 100.0 mL of 0.1 M HNO₃                              [ Select ]                       [“No, it will not result in a buffer solution.”, “Yes, it will result in a buffer solution.”]      

2) A 1.0 L solution initially contains 0.2 M CH₃COOH. Approximate the number of moles of CH₃COOH and CH₃COO⁻ in the solution after 0.1 mol of solid NaOH is added, and calculate the pH of the resulting solution. K_a of CH₃COOH is 1.8

×10⁻⁵.

1) The number of moles of CH₃COOH present is                            [ Select ]                       [“0.0”, “0.2”, “0.1”]         mol.

2) The number of moles of CH₃COO⁻ present is                            [ Select ]                       [“0.1”, “0.0”, “0.2”]         mol.

3) The pH of the resulting solution is                            [ Select ]                       [“4.44”, “4.74”, “5.05”]         .