AP Chemistry Review

Explain the difference between a strong acid and a weak acid.

• Strong acids fully dissociate, weak acids partially dissociate.

• Strong acids are blue, weak acids are red.

• Strong acids are positive, weak acids are negative.

• Strong acids are solid, weak acids are liquid.

What is the pH of a solution with a hydrogen ion concentration of 1 x 10^-3 M?

• 4

• 5

• 6

• 3

How does enthalpy change in an endothermic reaction?

• Enthalpy decreases

• Enthalpy increases

• Enthalpy remains constant

• Enthalpy becomes negative

Tags

NGSS.HS-PS1-4

Explain the concept of a buffer solution.

• A buffer solution is a solution that has no effect on pH when small amounts of acid or base are added.

• A buffer solution is a solution that only reacts with acid but not with base.

• A buffer solution is a solution that accelerates changes in pH when small amounts of acid or base are added.

• A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added.

If a reaction is at equilibrium and the concentration of reactants increases, what happens to the reaction?

• The reaction will produce more reactants to reestablish equilibrium.

• The reaction will produce more products to reestablish equilibrium.

• The equilibrium position remains unchanged.

• The reaction will be unable to reestablish equilibrium.

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

What is the role of a catalyst in a chemical reaction?

• A catalyst changes the products of the reaction.

• A catalyst speeds up the reaction by lowering the activation energy barrier.

• A catalyst slows down the reaction by increasing the activation energy barrier.

• A catalyst has no effect on the reaction rate.

Tags

NGSS.HS-PS1-5

Define the term 'equilibrium constant' and how it relates to chemical equilibrium.

• The equilibrium constant is the rate at which a reaction occurs

• The equilibrium constant is not affected by temperature changes

• The equilibrium constant is only applicable to reversible reactions

• The equilibrium constant relates the concentrations of products and reactants at equilibrium for a chemical reaction.

How does Gibbs free energy relate to spontaneity of a reaction?

• ΔG has no impact on the spontaneity of a reaction

• ΔG directly determines the rate of a reaction

• ΔG is only relevant for exothermic reactions

• ΔG determines whether a reaction is spontaneous (negative ΔG), non-spontaneous (positive ΔG), or at equilibrium (zero ΔG).

Explain the concept of dynamic equilibrium in a chemical reaction.

• Dynamic equilibrium occurs when the reaction stops completely.

• Dynamic equilibrium means the reaction proceeds in only one direction.

• Dynamic equilibrium only happens in irreversible reactions.

• Dynamic equilibrium in a chemical reaction is when the rate of the forward reaction equals the rate of the reverse reaction, maintaining constant concentrations of reactants and products.

If the equilibrium constant for a reaction is greater than 1, what does this indicate?

• The concentration of reactants is higher than that of products at equilibrium

• The concentration of products is higher than that of reactants at equilibrium

• The reaction does not reach equilibrium

• The reaction is exothermic