Question

 The acetic acid/acetate buffer system is a common buffer used in the laboratory.

 Write the equilibrium equation for the acetic acid/acetate buffer system. The formula of acetic acid is CH3CO2H.

 equilibrium equation:

 Which way does the equilibrium shift if more H₃O⁺ is added?

 The equilibrium will not change.

 The equilibrium will shift to the left.

 The equilibrium will shift to the right.

 Which way does the equilibrium shift if more OH^- is added?

 The equilibrium will shift to the right.

 The equilibrium will shift to the left.

 The equilibrium will not change.

 To prepare an acetic acid/acetate buffer, a technician mixes 30.5 mL of 0.0900 M acetic acid and 19.5 mL of 0.0900 M sodium acetate in a 100-mL volumetric flask and then dilutes the solution to the 100.00 mL mark. Determine the number of moles of acetic acid and the number of moles of sodium acetate in the buffer.

 moles of acetic acid =

 moles of sodium acetate =

 The concentration of H₃O⁺ in the buffer is 2.72 x 10^-5 M. What is the pH of the solution?

 pH=

Answer 1