Acidic environments accelerate corrosion in non-passivating metals

[cs_content][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ style=”margin: 0px;padding: 45px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]Shipwrecks and Salvage‎ > ‎6. Corrosion at Depths‎ > 

Explain that acidic environments accelerate corrosion in non-passivating metals[/cs_text][/cs_column][/cs_row][/cs_section][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ style=”margin: 0px;padding: 45px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]

  • The corrosion of non-passivating metals is accelerated in acidic environments when compared to basic or neutral environments.
  • The reduction of oxygen proceeds more rapidly at pH below 7:
pH ≥ 7: O2 + H2O + 4e– → 4OH– (0.4 V)

pH < 7: O2 + H+ + 4e– → 4OH– (1.23 V)

  • The second half-equation is more rapid due to its higher reduction potential.
  • The reduction of sulfate to sulfide is also accelerated in acidic environments.
  • Generally, seawater is slightly alkaline.
  • Acidic microclimates can form within seawater due to the activities of microorganisms and other chemical processes.
  • Around shipwrecks where there is an abundance of organic material for bacteria to feed upon, such acidic microclimates can form.
  • This would accelerate the corrosion of the shipwreck.
  • When pH is less than 3, hydrogen ions can directly oxidise passivating metals, such as iron:

Fe (s) + 2H+ → Fe2+ + H2 (g)

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