Types of Acids and Bases
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Arrhenius acids and bases
- Acids are hydrogen containing compounds that ionize to form hydrogen ions in aq solutions
- bases are compounds that ionize to produce hydroxide ions in aq solution.
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Arrhenius Acids
- Acids that contain only one ionizable hydrogen are called monoproticacids like HNO3,
- Acids that contain two ionizable hydrogen atoms are called diprotic acids like H2SO4,
- acids that contain three ionizable hydrogen atoms are triproticacids like H3PO4.
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Types of Ionizable Hydrogen's
- Only the hydrogens in very polar bonds are ionizable, which means that hydrogen is attached to a very electronegative element
- Methane has four hydrogen CH4 but they are attached by a very weak polar bonds so none of the hydrogens are ionizable, so methane is not an acid even though it contains hydrogen.
- In CH3COOH there is only one ionizable hydrogen (the one attached to the oxygen) so this is a monoprotic acid even though there are four hydrogens.
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Bronsted- Lowery acids and bases
- An acid is a hydrogen ion donor and a base is a hydrogen ion acceptor
- Ammonia is a base because when it is dissolved in water it accepts a hydrogen from the water to form ammonium ions and hydroxide ions.
- NH3 + H2O --> NH4+ + OH-
- In this reaction ammonia is the hydrogen ion acceptor and is therefore the Bronsted – Lowery base, water is the acid because it donates the hydrogen.
- This causes the hydroxide ion concentration to be larger than that of pure water, hence a basic solution.
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Conjugate Pairs
- In the reverse reaction ammonium is the acid and hydroxide is the base.
- This is known as a conjugate acid because it is the particle formed when a base gains a hydrogen ion and OH- is the conjugate base to water.
- For every Bronsted – lowery acid base pair there is always a conjugate base – acid pair.
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Lewis acids and bases
- An acid is a substance that can accept a pair of electrons and a base is a substance that donates a pair of electrons to form covalent bonds.
- A hydrogen ion can accept a pair of electrons to form a bond and is therefore a Lewis acid.
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Summary
Type Acids Bases
Arrhenius H+ producer OH - Producer
Bronsted –Lowry H+ Donor H+ Acceptor
Lewis Electron pair acceptor Electron pair donor
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