Question 1: Explain what acid rain is and how it differs from normal rain.

Answer: Acid rain is precipitation that has a pH lower than 5.6 due to dissolved acidic pollutants like sulfur dioxide and nitrogen oxides, which make it more acidic than normal rain.

Question 2: What are the primary pollutants responsible for acid rain?

Answer: Sulfur dioxide (SO2) and nitrogen oxides (NOx).

Question 1: Write the chemical equation showing how sulfur dioxide reacts with water in the atmosphere to form sulfuric acid.

Answer: SO2 + H2O → H2SO3 (sulfurous acid), which can further oxidize to form sulfuric acid (H2SO4).

Question 2: Describe how nitrogen oxides contribute to acid rain formation.

Answer: Nitrogen oxides (NO and NO2) react with water in the atmosphere to produce nitric acid (HNO3), contributing to acid rain.

Question 1: List three environmental effects of acid rain on ecosystems.

Answer: Damage to forests and crops, acidification of lakes and rivers harming aquatic life, deterioration of buildings and monuments.

Question 2: Describe one method industries use to reduce sulfur dioxide emissions.

Answer: Using flue gas desulfurization (scrubbers) to remove SO2 from emissions before they are released into the atmosphere.

Question 1: Calculate the pH of a rainwater sample with a hydrogen ion concentration of 1 x 10^-5 mol/L.

Answer: pH = -log[H+] = -log(1 x 10^-5) = 5.

Question 2: If normal rain has a pH of 5.6, how does a pH of 4.0 in a water sample indicate acid rain? Explain briefly.

Answer: A pH of 4.0 is more acidic than normal rain (pH 5.6), indicating the presence of pollutants that lower the pH, characteristic of acid rain.

Question 1: Identify two safety precautions to consider when handling sulfur dioxide in a laboratory setting.

Answer: Use in a well-ventilated area or fume hood, and wear protective goggles and gloves.

Question 2: Describe a simple experiment to demonstrate how sulfur dioxide forms sulfuric acid in the atmosphere, including the main variables involved.

Answer: Burn sulfur to produce SO2 gas, then expose it to water vapor in a controlled environment. Variables include sulfur amount (independent), water vapor presence (independent), and resulting acid concentration (dependent).