A 1.0 L buffer solution is 0.250 M HC₂H₃O₂ and 0.060 M NaC₂H₃O₂.Which of the following actions will destroy the buffer? A) adding 0.060 moles of NaC₂H₃O₂ B) adding 0.060 moles of HC₂H₃O₂ C) adding 0.060 moles of HCl D) adding 0.060 moles of KOH E) All of the above will destroy the buffer.

Question

Quizplus · Accepted Answer

Adding HCl will introduce additional H+ ions, which will react with the buffer's weak base component (H₂H₃O₂) to form more HC₂H₃O₂. This will decrease the pH of the buffer and destroy its ability to resist changes in pH. Option A and B involve adding more of the buffer's components, which will maintain the buffer capacity. Option D involves adding a strong base, which will react with the buffer's weak acid component to form more of the buffer's conjugate base, maintaining buffer capacity. Option E suggests all options would destroy the buffer which is not correct as seen above.

A 10 L Buffer Solution Is 0