Buffer Solutions and Their Functions

The video introduces buffer solutions, which resist pH changes when small amounts of substances are added. It explains the common ion effect and equilibrium in buffer systems, using acetic acid and sodium acetate as examples. The video details how equilibrium shifts affect pH and describes the components of buffer solutions, including weak acids and their conjugate bases. It also covers how buffers react with strong acids and bases, and how to identify buffer solutions from given pairs.

What is the primary function of a buffer solution?

• To completely dissociate in water

• To increase the pH of a solution

• To resist changes in pH

• To neutralize strong acids

When does a buffer solution stop working effectively?

• When the temperature is increased

• When large amounts of substances are added

• When the solution is diluted

• When small amounts of substances are added

What happens when sodium acetate is added to a solution of acetic acid?

• The solution becomes a strong acid

• A common ion effect is created

• The solution becomes neutral

• The pH decreases significantly

What is the common ion in the example of acetic acid and sodium acetate?

• Chloride ion

• Hydronium ion

• Sodium ion

• Acetate ion

What is the role of sodium in the sodium acetate and acetic acid buffer system?

• It increases the pH

• It neutralizes the solution

• It is a spectator ion

• It acts as a reactant

What happens to the hydronium ion concentration when the equilibrium shifts to the left?

• It remains the same

• It increases

• It decreases

• It becomes neutral

What must a buffer solution contain?

• A neutral salt and water

• A strong base and its conjugate acid

• A weak acid and its conjugate base

• A strong acid and a strong base

Why do buffer solutions resist changes in pH?

• Because they are diluted

• Because they are highly concentrated

• Because they contain a weak acid and a weak base that do not react with each other

• Because they contain a strong acid and a strong base

Which of the following pairs will make a buffer solution?

• Hydrochloric acid and sodium acetate

• Sodium hydroxide and sodium chloride

• Nitric acid and sodium nitrate

• Ammonia and ammonium bromide

What is an exception to the rule for forming buffer solutions?

• Using a neutral salt and water

• Using a strong acid and a strong base

• Using a weak acid and a weak base

• Forcing a reaction to form a buffer under the right circumstances