Acid-Base Equilibria

What is the definition of an acid according to the Arrhenius theory?

• A substance that dissociates in water to produce hydrogen ions (H+).

• A substance that releases hydroxide ions (OH-) in water

• A substance that is neutral in nature

• A compound that forms salts when reacting with bases

Explain the concept of pH and how it is related to the concentration of H+ ions in a solution.

• pH is related to the concentration of O- ions in a solution

• pH is a measure of temperature in a solution

• pH is only applicable to solid substances

• pH is a measure of acidity or basicity related to the concentration of H+ ions in a solution.

What is the difference between a strong acid and a weak acid?

• Strong acids have a lower concentration than weak acids

• Strong acids are less corrosive than weak acids

• Weak acids have a higher pH than strong acids

• Strong acids completely dissociate in water, while weak acids only partially dissociate.

Describe the process of neutralization and give an example.

• An example of neutralization is the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) to form water (H2O) and sodium chloride (NaCl). The balanced chemical equation for this reaction is: HCl + NaOH -> H2O + NaCl

• Neutralization involves the formation of carbon dioxide and water.

• An example of neutralization is the reaction between sulfuric acid and potassium hydroxide.

• Neutralization is the process of combining an acid and a base to form a salt and water.

What is the pH range for acidic solutions?

• 2 to 6.99

• 0 to 8.99

• 0 to 6.99

• 1 to 7.99

How does the pH scale indicate the acidity or basicity of a solution?

• The pH scale indicates the acidity or basicity of a solution based on the concentration of hydrogen ions. A pH below 7 is acidic, a pH of 7 is neutral, and a pH above 7 is basic.

• A pH of 7 is acidic

• The pH scale measures the temperature of the solution

• The pH scale is based on the color of the solution

Define the term 'buffer solution' and explain its importance.

• A buffer solution is a type of cleaning solution used in households

• A buffer solution is only used in industrial applications

• A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added. It consists of a weak acid and its conjugate base, or a weak base and its conjugate acid. Buffers are important in maintaining stable pH levels in various chemical and biological processes.

• A buffer solution is a solution with a high concentration of a single acid or base

What is the role of conjugate acid-base pairs in maintaining equilibrium?

• Conjugate acid-base pairs cause pH imbalance in a solution

• Conjugate acid-base pairs help in stabilizing the pH of a solution by accepting or donating protons to maintain equilibrium.

• Conjugate acid-base pairs have no role in maintaining equilibrium

• Conjugate acid-base pairs are only relevant in acidic solutions

Explain the significance of the equilibrium constant (Ka or Kb) in acid-base reactions.

• The equilibrium constant (Ka or Kb) measures the rate of the acid-base reaction

• Ka or Kb is used to determine the color change in acid-base reactions

• The equilibrium constant (Ka or Kb) in acid-base reactions quantifies the strength of an acid or base by measuring the ratio of products to reactants when the reaction reaches equilibrium.

• The equilibrium constant (Ka or Kb) indicates the volume of the acid or base used in the reaction

Discuss the common ion effect and its impact on the ionization of weak acids and bases.

• The common ion effect decreases the ionization of weak acids and bases by shifting the equilibrium towards the non-ionized form.

• The common ion effect has no impact on the ionization of weak acids and bases.

• The common ion effect increases the ionization of weak acids and bases by shifting the equilibrium towards the ionized form.

• The common ion effect only affects strong acids and bases, not weak ones.