[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]The Acidic Environment > 3. Acids >
Define acids as proton donors and describe the ionisation of acids in water[/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 Lowry-Bronsted theory defines an acid as a substance that acts as a proton donor.
- When an acid molecule is in water, it can ionise, releasing a proton, or hydrogen ion, and forming a negative ion.
- The proton, or hydrogen ion, is donated to a water molecule, forming a hydronium ion:
- For example, in the case of hydrochloric acid:
- Acids can be classified according to their potential for proton donation per molecule:
- Monoprotic acids: Acids that can release only one proton, or hydrogen ion, per molecule.
- Diprotic acids: Acids that can release up to two protons, or hydrogen ions, per molecule.
- Triprotic acids: Acids that can release up to three protons, or hydrogen ions, per molecule.
Ionisation/Dissociation of acetic acid in water (click to enlarge)
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