Advanced Concepts

Question 1

Discuss the concept the buffer capacity

Answer 1

Buffer capacity quantities the ability of a solution to resist changes in pH by either absorbing or desorbing H+ and OH- ions

Question 2

Explain how a polyprotic acid can form a buffer

Answer 2

Polyprotic acids donates more than one proton per molecule which can form buffers when they are moved with their conjugate base.

Question 3

Describe the limitations of the Henderson-Hasselbalch equation

Answer 3

The assumption stated in the Henderson equation might not be applicable when associating with strong bases or acids. The most important assumption in this equation is that the concentrations of acid and conjugate bases always stay constant during equilibrium

Question 4

Explain the role of water as an acid and a base in pH calculations

Answer 4

Water acts as a base when combined with a stronger acid. Water acts as an acid when combined with a strong base such as ammonia.

Question 5

Discuss the impact of temperature on the dissociation of acids and bases

Answer 5

If dissolution is exothermic, the dissociation constant will rise with increasing temperature. if dissolution is endothermic, H stood evaluatively using le chatelier principle. When the reaction is endothermic, Ka increases and pKa drops with increasing temperatures. When the reaction is exothermic, Ka increases and pKa reduces with increasing temperature. The degree of dissociation increases with increase in temperature.