What happens to the pH of the environment around the cathode during cathodic protection?

What happens to the pH of the environment around the cathode during cathodic protection?

• A. It becomes more acidic
• B. It becomes more alkaline
• C. It remains neutral
• D. It fluctuates unpredictably

Answer: (B)

During cathodic protection, the pH of the environment around the cathode tends to become more alkaline. This occurs due to the reduction reactions that take place at the cathode, in which hydrogen ions (H+) in the environment are consumed. As these hydrogen ions are reduced, they form hydrogen gas, thereby decreasing the concentration of H+ ions in the solution. This change increases the ratio of hydroxide ions (OH-) compared to H+ ions, which leads to a more basic (alkaline) environment. The generation of hydroxide ions is crucial in cathodic protection systems, as it mitigates corrosion by changing the local chemistry around the cathode, ultimately reducing the corrosion rate of the protected metal. The other options do not accurately reflect what occurs during cathodic protection. An increase in acidity, for example, would imply a higher concentration of H+ ions, which is contrary to the reduction processes that diminish H+ concentration, thus making the pH more alkaline. As for neutrality and unpredictability, those would not describe the specific chemical interactions happening in a controlled cathodic protection environment, where conditions are typically managed to achieve a stable outcome.

During cathodic protection, the pH of the environment around the cathode tends to become more alkaline. This occurs due to the reduction reactions that take place at the cathode, in which hydrogen ions (H+) in the environment are consumed. As these hydrogen ions are reduced, they form hydrogen gas, thereby decreasing the concentration of H+ ions in the solution.

This change increases the ratio of hydroxide ions (OH-) compared to H+ ions, which leads to a more basic (alkaline) environment. The generation of hydroxide ions is crucial in cathodic protection systems, as it mitigates corrosion by changing the local chemistry around the cathode, ultimately reducing the corrosion rate of the protected metal.

The other options do not accurately reflect what occurs during cathodic protection. An increase in acidity, for example, would imply a higher concentration of H+ ions, which is contrary to the reduction processes that diminish H+ concentration, thus making the pH more alkaline. As for neutrality and unpredictability, those would not describe the specific chemical interactions happening in a controlled cathodic protection environment, where conditions are typically managed to achieve a stable outcome.