what is an electrolyte
Key Terms
what is an electrolyte
Under what two circumstances in which ionic compounds can conduct electricity/ act as electrolytes
Answer: If dissolved in water/ solution, If molten
how can an electric current be conducted through an electrolyte
Answer: ions are available and free to move
what is electrolysis
Answer: the passing of electricity through an electrolyte to cause a chemical reaction
what is an electrode
Answer: a solid material that conducts electricity
what occurs at the cathode
Answer: reduction
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| Term | Definition |
|---|---|
what is an electrolyte | Answer: a substance that conducts electricity when dissolved in water or molten |
Under what two circumstances in which ionic compounds can conduct electricity/ act as electrolytes | Answer: If dissolved in water/ solution, If molten |
how can an electric current be conducted through an electrolyte | Answer: ions are available and free to move |
what is electrolysis | Answer: the passing of electricity through an electrolyte to cause a chemical reaction |
what is an electrode | Answer: a solid material that conducts electricity |
what occurs at the cathode | Answer: reduction |
what occurs at the anode | Answer: oxidation |
describe the observations seen (using green copper (II) chromate solutions) Demonstrating the movement of ions when connected to an electrical current | Answer: Observation: a yellow colour will migrate towards the anode and a blue colour will migrate towards the cathode. The yellow colour caused by the chromate ions. The blue colour is caused by the copper (II) ions |
Inert electrodes reaction | Answer: electrodes do not react with the electrolyte in which they are placed |
Active electrodes reactions | Answer: electrodes that react with the electrolyte in which they are placed |
Inert electrodes suitable to use for these electrolysis | Answer: Platinum Graphite (Carbon) |
Active electrodes suitable to use for these electrolysis | Answer: Copper electrodes |
H2O will always reduce before the following ions | Answer: So4 2-, Na+, K+ |
what was the result/ Observation Electrolysis of acidified water (H2o + H+) using inert electrodes | Answer: Bubbles of Hydrogen gas will collect over the cathode, Bubbles of oxygen gas will collect over the anode the volume of hydrogen will always be double the amount of oxygen formed (1 mole of hydrogen formed for every half mole oxygen formed) |
Balanced chemical equation for reaction at cathode Electrolysis of acidified water (H2o + H+) using inert electrodes | Answer: 2H+ + 2e- → H2↑ |
balanced chemical equation for reaction at anode Electrolysis of acidified water (H2o + H+) using inert electrodes | Answer: H2O - 2e- → 2H+ + 1/2O2↑ |
Describe the reaction/ result Electrolysis of sodium sulfate (NaSO4) using inert electrodes | Answer: Bubbles of hydrogen gas will collect over the cathode. The universal indicator turns from green to blue at the cathode. Bubbles of oxygen gas collect over the anode. The universal indicator turns from green to red at the cathode the volume of hydrogen will always be double the amount of oxygen formed (1 mole of hydrogen formed for every half mole oxygen formed) |
Balanced chemical equation describing the reaction at the Cathode Electrolysis of sodium sulfate (NaSO4) using inert electrodes | Answer: 2H2O - 2e- → H2↑ + 2OH- |
Balanced chemical equation describing the reaction at the anode Electrolysis of sodium sulfate (NaSO4) using inert electrodes | Answer: H2O - 2e- → 2H+ + 1/2O2↑ |
list the reactions and observations Electrolysis of potassium iodide (KI) solution using inert electrodes | Answer: Bubbles of Hydrogen gas will collect over the cathode Phenolphthalein turns from colourless to pink at the cathode A red-brown colour will form at the anode due to the formation of iodine (I2) |
Write a balanced equation for the reaction that occurs at the cathode Electrolysis of potassium iodide (KI) solution using inert electrodes | Answer: 2H2O - 2e- → H2↑ + 2OH- |
Write a balanced equation for the reaction that occurs at the anode Electrolysis of potassium iodide (KI) solution using inert electrodes | Answer: 2I- - 2e- → I2 |
Describe the result/ observation Electrolysis of aqueous copper sulfate (CUSO4) using active electrodes | Answer: The pure copper cathode increases in mass as the Cu 2+ ions in solution are reduced to Cu. The impure copper anode is ‘eaten away’ and decreases in mass and the Cu atoms in the anode are oxidised to CU 2+. Impurities are undissolved and fall to the bottom of the beaker under the anode |
describe the reaction at the cathode Electrolysis of aqueous copper sulfate (CUSO4) using active electrodes | Answer: Cu 2+ +2e- → Cu↓ |
Describe the reaction at the anode | Electrolysis of aqueous copper sulfate (CUSO4) using active electrodes | Answer: Cu - 2e- → CU2+ |
Give two applications of using electrolysis using active electrodes | Answer: Purification of copper Electroplating |
give two examples of electroplating | Answer: cutlery electroplated with silver Bath fittings plated in nickel and chromium |
give two advantages to electroplating one metal with another | Answer: the object appears more attractive The object is more resistant to corrosion |