Question 1: Aqueous electrolysis involves passing an electric current through a solution containing water and dissolved substances, causing chemical reactions at the electrodes. These reactions depend on the ions present in the solution and their tendencies to gain or lose electrons.

Answer: Aqueous electrolysis uses water and dissolved ions; electric current causes chemical reactions at electrodes based on ion tendencies.

Question 1: Define electrolysis.

Answer: Electrolysis is a chemical process where an electric current causes a non-spontaneous chemical reaction to occur, typically breaking down compounds into their elements or ions.

Question 2: Explain why water undergoes electrolysis and what products are formed at the electrodes.

Answer: Water undergoes electrolysis because it contains ions that can be reduced or oxidized; hydrogen gas forms at the cathode, and oxygen gas forms at the anode.

Question 3: List the ions typically involved in aqueous electrolysis of a salt solution.

Answer: Common ions include H⁺, OH⁻, Cl⁻, Na⁺, SO₄²⁻, and other anions and cations from dissolved salts.

Question 1: Calculate the volume of hydrogen gas produced at the cathode when 2.0 Amperes of current is passed through water for 30 minutes. (Use Faraday's constant: 96485 C/mol; 1 mol of H₂ gas occupies 22.4 L).

Answer: V = 22.4 L/mol * (2.0 A * 1800 sec) / (2 * 96485 C/mol) = 0.42 liters

Question 2: If 0.5 mol of sodium chloride solution is electrolyzed, how much chlorine gas (Cl₂) is produced at the anode? (Molar mass of Cl₂ = 70.9 g/mol).

Answer: Chlorine produced = 0.5 mol * 1 mol Cl₂ / 1 mol NaCl = 0.5 mol; mass = 0.5 mol * 70.9 g/mol = 35.45 grams

Question 1: Outline the steps to set up an aqueous electrolysis experiment using a salt solution.

Answer: Prepare a solution of salt in water, connect electrodes to a power supply, immerse the electrodes in the solution without touching, ensure proper insulation, and turn on the power. Always wear safety goggles and gloves, and work in a well-ventilated area to avoid inhaling gases.

Question 1: During electrolysis of a copper sulfate solution, students observe that copper metal deposits on the cathode, and bubbles of oxygen are released at the anode. Explain the electrochemical processes occurring at both electrodes.

Answer: At the cathode, Cu²⁺ ions gain electrons (reduction) to form copper metal. At the anode, water molecules lose electrons (oxidation) to produce oxygen gas and H⁺ ions.

Question 1: Describe the process of aqueous electrolysis of sodium chloride solution and identify the products formed at both electrodes.

Answer: When sodium chloride solution undergoes electrolysis, sodium ions migrate toward the cathode where they gain electrons to form sodium metal (if conditions allow) or react with water to produce sodium hydroxide and hydrogen gas. Chloride ions migrate toward the anode, where they lose electrons to form chlorine gas. Alternatively, water oxidation can produce oxygen gas, depending on the electrode potentials and solution conditions.

Question 1: Provide an example of an industry process that uses aqueous electrolysis and describe its significance.

Answer: Electrolysis is used in metal refining, such as purifying aluminum from bauxite ore, which is essential for producing high-purity metals for manufacturing.