Acid-Base Equilibrium

Mr. Anderson explains acid-base equilibrium, focusing on the reversible nature of reactions and the role of equilibrium constants. He discusses the importance of water in these reactions, highlighting its amphoteric properties. The video covers the difference between strong and weak acids/bases, using equilibrium constants to determine their strength. Neutralization reactions and titration curves are also explained, illustrating how pH changes during these processes. The video aims to clarify these concepts, making them more accessible to students.

What is the equilibrium constant a measure of in a chemical reaction?

• The amount of energy released

• The speed of the reaction

• The ratio of products to reactants at equilibrium

• The temperature at which the reaction occurs

In acid-base chemistry, what role does a proton donor play?

• It neutralizes the reaction

• It increases the pH

• It acts as an acid

• It acts as a base

What is the significance of water being amphoteric?

• It can only act as an acid

• It is neutral and does not participate in reactions

• It can only act as a base

• It can act as both an acid and a base

What is the equilibrium constant of water (Kw) at 25°C?

• 1 x 10^-10

• 1 x 10^-4

• 1 x 10^-14

• 1 x 10^-7

How is the strength of an acid determined?

• By its equilibrium constant (Ka)

• By its color

• By its molecular weight

• By its boiling point

Which of the following is a characteristic of a strong acid?

• It has a low Ka value

• It does not donate protons

• It has a high Ka value

• It is always a solid

What is a polyprotic acid?

• An acid that can donate one proton

• An acid that can donate two or more protons

• An acid that cannot donate protons

• An acid that is always weak

What happens at the equivalence point in a titration of a strong acid with a strong base?

• The pH is greater than 7

• The pH is exactly 7

• The pH is less than 7

• The solution becomes solid

In a titration of a weak acid with a strong base, what is formed during the buffering region?

• A strong acid

• A strong base

• A conjugate base

• A neutral solution

What principle explains the stabilization of pH in a buffer solution?

• Newton's third law

• Boyle's law

• Le Chatelier's principle

• Avogadro's law