What Are Acids And Bases?
- types of compounds that have characteristic formulas and similar chemical behaviours
- very important reactants and catalysts in industrial processes
- the product of an acid and base is usually salt and water
Daily Examples
-Acids:
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vinegar
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lemon juice
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battery acid
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Coca-cola®
-Bases
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baking soda
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ammonia
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toothpaste
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Windex®
Characteristics of Acids and Bases
Acids: |
Bases: |
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- bitter tasting, slippery in aqueous solution
- good conductors due to OH-‐ion
- turn red litmus paper blue
- turn phenolphthalein indicator pink
- formulas often contain a hydroxide ion (OH‐) or a bicarbonate group (HCO3)
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Theories
The Arrhenius Theory
- According to the Arrhenius theory, all acids release hydrogen ions (H+) when dissolved in water. For example: HCl + H2O à H+(aq) + Cl-(aq)
- According to the theory, all bases release hydroxide ions (OH-‐) when dissolved in water. For example: NaOH + H2O à Na+(aq) + OH-(aq)
Strong Acids & Bases vs. Weak Acids & Bases
Acids and bases are often referred to as strong or weak.
Acids:
-A strong acid dissociates completely in water. This means that none of the acid is left in solution; rather, 100% of the acid ionizes into a hydrogen ion (H+) and an anion.
-A weak acid does not dissociate completely in aqueous solution.
There are six common strong acids:
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HCl -hydrochloric acid
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HNO3 -nitric acid
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H2SO4 -sulfuric acid
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HBr -hydrobromic acid
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HI -hydroiodic acid
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HClO4 -perchloric acid
Bases:
-A strong base dissociates completely in water to form hydroxide ions (OH-) and a cation.
-A weak base does not dissociate completely in aqueous solution.
There are six common strong bases:
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LiOH -lithium hydroxide
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NaOH -sodium hydroxide
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KOH -potassium hydroxide
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Ca(OH)2 -calcium hydroxide
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Sr(OH)2 -strontium hydroxide
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Ba(OH)2 -barium hydroxide
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