Question 1: Define a strong acid and a weak acid. Explain the main difference between their dissociation in water.

Answer: A strong acid completely dissociates into ions in water, whereas a weak acid only partially dissociates, resulting in a dynamic equilibrium between dissociated and undissociated molecules.

Question 2: Which of the following acids is typically classified as a strong acid? a) Hydrochloric acid (HCl), b) Acetic acid (vinegar), c) Carbonic acid.

Answer:

Question 3: Fill in the blank: The pH of a strong acid solution is generally __________ than that of a weak acid solution of the same concentration.

Answer: lower

Question 1: Describe the process of dissociation of hydrochloric acid (HCl) in water.

Answer: Hydrochloric acid dissociates completely in water, breaking into hydrogen (H⁺) ions and chloride (Cl⁻) ions, resulting in a high concentration of H⁺ ions and a low pH.

Question 2: Explain why acetic acid (vinegar) is considered a weak acid, including its behavior in water.

Answer: Acetic acid only partially dissociates in water, establishing an equilibrium between undissociated molecules and ions, resulting in a higher pH compared to strong acids.

Question 1: Calculate the pH of a 0.01 M hydrochloric acid (HCl) solution. (Use pH = -log[H⁺])

Answer: 2

Question 2: If the pH of a solution is 3, what is the concentration of hydrogen ions [H⁺] in mol/L?

Answer: 1.0 x 10^{-3}

Question 1: Describe a safety precaution that should be taken when handling concentrated hydrochloric acid in a laboratory setting.

Answer: Wearing appropriate PPE such as gloves, goggles, and a lab coat, and working in a well-ventilated area to avoid inhalation of fumes.

Question 2: Provide an example of a practical use for weak acids in industry or daily life.

Answer: Vinegar, which contains acetic acid, is used in cooking and food preservation.

Question 3: Explain why industries prefer using weak acids for certain processes instead of strong acids.

Answer: Industries prefer weak acids in some processes because they are less corrosive and safer to handle, reducing the risk of damage to equipment and harm to workers, while still providing the necessary chemical properties for specific reactions.

Question 1: A solution of acetic acid has a concentration of 0.1 M and a pH of 2.9. Explain what this indicates about its dissociation behavior compared to a typical weak acid.

Answer: This indicates that the acetic acid partially dissociates, resulting in a pH slightly higher than that of a strong acid at the same concentration, showing its weak acid nature with limited ionization.